State Boyle's law.

What are ideal gases? In what way real gases differ from ideal gases.

Suggest why there is no hydrogen (H₂) in our atmosphere. Why does the moon have no atmosphere?

When the driver of an automobile applies brake, the passengers are pushed toward the front of the car but a helium balloon is pushed toward back of the car. Upon forward acceleration the passengers are pushed toward the front of the car. Why?

A sample of gas at 15°C at 1 atm. has a volume of 2.58 dm³. When the temperature is raised to 38°C at 1 atm does the volume of the gas increase? If so, calculate the final volume.

State the various statements of second law of thermodynamics.

30.4 kJ is required to melt one mole of sodium chloride. The entropy change during melting is 28.4 JK^-1 mol^-1. Calculate the melting point of sodium chloride.

Calculate the enthalpy of hydrogenation of ethylene from the following data. Bond energies of C - H, C - C , C = C and H - H are 414, 347, 618 and 435 kJ mol^-1

The standard enthalpies of formation of SO₂ and SO₃ are -297 kJ mol^-1 and -396 kJ mol^-1 respectively. Calculate the standard enthalpy of reaction for the reaction: SO₂ + \(\frac{1}{2}\)O₂⟶SO₃

Find out the value of equilibrium constant for the following reaction at 298K; 2NH_3(g)+ CO_2(g) \(\rightleftharpoons \) NH₂CONH_2(aq) + H₂O(I) Standard Gibbs energy change, \(\Delta { G }_{ r }^{ 0 }\) at the given temperature is -13.6 kJ mol^-1.

What are state and path functions? Give two examples

Enthalpy of neutralization is always a constant when a strong acid is neutralized by a strong base: account for the statement

State the various statements of second law of thermodynamics.

1 mole of an ideal gas, maintained at 4.1 atm and at a certain temperature, absorbs heat 3710 J and expands to 2 litres. Calculate the entropy change in expansion process.

Cyanamide (NH₂CN) is completely burnt in excess oxygen in a bomb calorimeter, ΔU was found to be -742.4 kJ mol^-1calculate the enthalpy change of the reaction at 298K. NH₂CN_(S) +\(\frac{3}{2}\)O_2(g)⟶ N_2(g)+ CO_2(g)+ H₂O(I) ΔH= ?

The value of Kc for the reaction
N₂O₂(g) \(\rightleftharpoons \) 2NO₂(g)

The equilibrium concentrations of NH₃, N₂ and H₂ are 1.8 x 10^-2 M, 1.2 x 10^-2 M and 3 x 10^-2 M respectively. Calculate the equilibrium constant for the formation of NH₃ from N₂ and H₂. [Hint: M= mol lit^-1]

For the reaction,
A₂(g) + B₂(g) ⇌ 2AB(g) ; ΔH is –ve.
the following molecular scenes represent different reaction mixture (A – green, B – blue)

i) Calculate the equilibrium constant K_P and (K_C).
ii) For the reaction mixture represented by scene (x), (y) the reaction proceed in which directions?
iii) What is the effect of increase in pressure for the mixture at equilibrium.

For the reaction
SrCO₃ (s) ⇌ SrO (s) + CO₂(g),
the value of equilibrium constant K_P = 2.2 x 10^–4 at 1002 K. Calculate K_C for the reaction.

Oxidation of nitrogen monoxide was studied at 200^o C with initial pressures of 1 atm NO and 1 atm of O₂. At equilibrium partial pressure of oxygen is found to be 0.52 atm calculate K_P value.

The value of K_c for the following reaction at 717 K is 48.

One mole of H₂ and one mole of I₂ are allowed to attain equilibrium in 1 lit container. If the equilibrium mixture contains 0.4 mole of HI. Calculate the equilibrium constant.

For an equilibrium reaction K_p = 0.0260 at 25° C ΔH= 32.4 kJmol^-1, calculate Kp at 37° C

One mole of PCl₅ is heated in one litre closed container. If 0.6 mole of chlorine is found at equilibrium, calculate the value of equilibrium constant.

To study the decomposition of hydrogen iodide, a student fills an evacuated 3 litre flask with 0.3 mol of HI gas and allows the reaction to proceed at 500^o C. At equilibrium he found the concentration of HI which is equal to 0.05 M. Calculate K_C and K_{P for this reaction.}

Vapour pressure of a pure liquid A is 10.0 torr at 27°C. The vapour pressure is lowered to 9.0 torr on dissolving one gram of B in 20 g of A. If the molar mass of A is 200 then calculate the molar mass of B.

0.75 g of an unknown substance is dissolved in 200 g water. If the elevation of boiling point is 0.15 K and molal elevation constant is 7.5 K Kg mol^-1 then, calculate the molar mass of unknown substance

2g of a non electrolyte solute dissolved in 75 g of benzene lowered the freezing point of benzene by 0.20 K. The freezing point depression constant of benzene is 5.12 K Kg mol^-1. Find the molar mass of the solute.

The depression in freezing point is 0.24K obtained by dissolving 1g NaCl in 200g water. Calculate van’t-Hoff factor. The molal depression constant is 1.86 K Kg mol^-1.

The observed depression in freezing point of water for a particular solution is 0.093^o C. Calculate the concentration of the solution in molality. Given that molal depression constant for water is 1.86 K Kg mol^-1.

If 5.6 g of KOH is present in
(a) 500 mL and
(b) 1 litre of solution 
Calculate the molarity of each of these solutions.

What volume of 4M HCl and 2M HCl should be mixed to get 500 mL of 2.5 M HCl ?

0.24 g of a gas dissolves in 1 L of water at 1.5 atm pressure. Calculate the amount of dissolved gas when the pressure is raised to 6.0 atm at constant temperature.

An aqueous solution of 2% nonvolatile solute exerts a pressure of 1.004 bar at the boiling point of the solvent. What is the molar mass of the solute when P_A is 1.013 bar ?

Ethylene glycol (C₂H₆O₂) can be at used as an antifreeze in the radiator of a car. Calculate the temperature when ice will begin to separate from a mixture with 20 mass percent of glycol in water used in the car radiator. K_f for water = 1.86 K Kg mol^-1 and molar mass of ethylene glycol is 62 g mol^-1.

Write structural formula for the following compounds
(i) Cyclohexa-1, 4-diene
(ii) Ethynyl cyclohexane.

Write all the possible isomers of molecular formula C₄H₁₀O and identify the isomerisms found in them.

0.16 g of an organic compound was heated in a carius tube and H₂SO₄ acid formed was precipitated with BaCl₂. The mass of BaSO₄ was 0.35g. Find the percentage of sulphur [30.04]

0.40 g of an iodo-substituted organic compound gave 0.235 g of AgI by carius method. Calculate the percentage of iodine in the compound. (Ag = 108, I = 127)

0.33 g of an organic compound containing phosphorous gave 0.397 g of Mg₂P₂O₇ by the analysis. Calculate the percentage of P in the compound.

Dissolved oxygen in water is responsible for aquatic life. What processes are responsible for the reduction in dissolved oxygen in water ?

From where does ozone come in the photo chemical smog ?

Even though the use of pesticides increases the crop production, they adversely affect the living organisms. Explain the function and the adverse effects of the pesticides.

Explain how oxygen deficiency is caused by carbon monoxide in our blood ? Give its effect

What are the various methods you suggest to protect our environment from pollution ?

Calculate the molar mass of the following compounds. 
i) urea [CO(NH₂)₂]
ii) Acetone [CH₃ COCH₃]
iii) Boric Acid [H₃ BO₃]
iv) Sulphuric  Acid [H₂ SO₄]

The reaction between aluminium and ferric oxide can generate temperatures up to 3273 K and is used in welding metals. (Atomic mass of AC = 27 u atomic mass of O = 16 u )
2Al + Fe₂O₃ \(\longrightarrow \) Al₂O₃ + 2Fe;  If in this process, 324 g of aluminum is allowed to react with 1.12 kg of ferric oxide
i) Calculate the mass of Al₂O₃ formed
ii) How much of the excess reagent is left at the end of the reaction ?

A Compound on analysis gave Na = 14.31% S = 9.97% H = 6.22% and 0 = 69.5%.
Calculate the molecular formula of the compound if all the hydrogen in the compound is present in combination with oxygen as a water of crystallization. (molecular mass of the compound is 322).

Balance the following equations by ion electron method.
i) \({ KMn }O_{ 4 }+{ SnCl }_{ 2 }+HCI\longrightarrow MnCI_{ 2 }+{ SnCI }_{ 4 }+{ H }_{ 2 }O+KCI\)
ii) 
iii) 
iv) 

Calculate the percentage composition of the elements present in magnesium carbonate. How many kilogram of CO₂ can be obtained by heating 1 kg of 90 % pure magnesium carbonate.

An ion with mass number 37 possesses unit negative charge. If the ion contains 11.1% more neutrons than electrons, Find the symbol of the ion.

Calculate the energy required for the process.
\({ He }_{ (g) }^{ + }\longrightarrow { He }_{ (g) }^{ 2+ }+{ e }^{ - }\)
The ionisation energy for the H atom in its ground state is -13.6 ev atom^-1

Protons can be accelerated in particle accelerators. Calculate the wavelength (in Å) of such accelerated proton moving at 2.85 x 10⁸ ms^-1 (the mass of proton is 1.673 x 10^-27 Kg).

Suppose that the uncertainty in determining the position of an electron in an orbit is 0.6 \(\mathring{A}\) . What is the uncertainty in its momentum

What is the de Broglie wave length of an electron, which is accelerated from the rest, through a potential difference of 100 V ?

The Li²⁺ ion is a hydrogen like ion that can be described by the Bohr model. Calculate the Bohr radius of the third orbit and calculate the energy of an electron in 4^th orbit.

Protons can be accelerated in particle accelerators. Calculate the wavelength (in Å) of such accelerated proton moving at 2.85 x 10⁸ ms^-1 (the mass of proton is 1.673 x 10^-27 Kg).

What is the de Broglie wavelength (in cm) of a 160 g cricket ball travelling at 140 Km hr ^-1.

Show that if the measurement of the uncertainty in the location of the particle is equal to its de Broglie wavelength, the minimum uncertainty in its velocity is equal to its velocity 1/4\(\pi\) of its velocity (V).

Identify the missing quantum numbers and the sub energy level

Explain the periodic trend of ionisation potential.

Why the first ionisation enthalpy of sodium is lower than that of magnesium while its second ionisation enthalpy is higher than that of magnesium.

By using paulings method calculate the ionic radii of K⁺ and CI^- ions in the potassium chloride crystal. Given that dk⁺-cl^-=3.14 Å. 

Explain the following, give appropriate reasons.
(i) Ionisation potential of N is greater than that of O.
(ii) First ionisation potential of C-atom is greater than that of B atom, where as the reverse is true is for second ionisation potential.
(iii) The electron affinity values of Be, Mg and noble gases are zero and those of N (0.02 eV) and P (0.80 eV) are very low.
(iv) The formation of F-(g) from F(g) is exothermic while that of O^2-(g) from O (g) is endothermic.

State the trends in the variation of electronegativity in group and periods.

Justify the position of hydrogen in the periodic table?

Explain preparation of hydrogen using electrolysis.

A group-1 metal (A) which is present in common salt reacts with (B) to give compound (C) in which hydrogen is present in –1 oxidation state. (B) on reaction with a gas (C) to give universal solvent (D). The compound (D) on reacts with (A) to give (E), a strong base. Identify A, B, C, D and E. Explain the reactions.

An isotope of hydrogen (A) reacts with diatomic molecule of element which occupies group number 16 and period number 2 to give compound (B) is used as a moderator in nuclear reaction. (A) adds on to a compound ( C), which has the molecular formula C₃H₆ to give (D). Identify A, B, C and D.

Compare the structures of H₂O and H₂O₂ .

Give the uses of gypsum.

Discuss briefly the similarities between beryllium and aluminium.

Alkaline earth metal (A), belongs to 3rd period reacts with oxygen and nitrogen to form compound (B) and (C) respectively. It undergo metal displacement reaction with AgNO₃ solution to form compound (D).

Explain the important common features of Group 2 elements.

Describe briefly the biological Importance of Calcium and magnesium.

How would you know whether a redox reaction is taking place in an acidic, alkaline or neutral medium?

What is the most essential conditions that must be satisfied in a redox reaction?

Why is anode called oxidation electrode, whereas the cathode is called reduction electrode?

Zn rod is immersed in CuSO₄ solution. What will you observe after an hour? Explain you observation in terms of the redox reaction.

Nitric acid is an oxidising agent and reacts with PbO but it does not react with PbO₂ Explain why?

Explain the following observation
Aerated water bottles are kept under water during summer

Explain whether a gas approaches ideal behavior or deviates from ideal behaviour if
it is compressed to a smaller volume at constant temperature.

Write the Van der Waals equation for a real gas. Explain the correction term for pressure and volume.

Derive the values of critical constants in terms of van der Waals constants.

Calculate the work done when 2 moles of an ideal gas expands reversibly and isothermally from a volume of 500 ml to a volume of 2 L at 25°C and normal pressure.

Calculate the standard heat of formation of propane, if its heat of combustion is -2220.2 kJ mol^-1. the heats of formation of CO_2(g) and H₂O(l) are -393.5 and -285.8 kJ mol^-1 respectively

For the reaction Ag₂O_(s) ⟶2Ag_(s) + \(\frac{1}{2}\)O_2(g) : ΔH =30.56 kJ mol^-1 and AS = 6.66JK^-1 mol^-1 (at 1 atm). Calculate the temperature at which ΔG is equal to zero. Also predict the direction of the reaction (i) at this temperature and (ii) below this temperature.

Calculate the enthalpy change for the reaction
Fe₂O₃ + 3CO ⟶ 2Fe + 3CO₂ from the following data.
2Fe +\(\frac{3}{2}\)O₂ ⟶ Fe₂O₃; ΔH = -741 kJ
C +\(\frac{1}{2}\)O₂ ⟶ CO; ΔH = -137 kJ 
C + O₂ ⟶ CO₂; ΔH = - 394.5 kJ

A gas mixture of 3.67 lit of ethylene and methane on complete combustion at 25°C and at 1 atm pressure produce 6.11 lit of carbondioxide. Find out the amount of heat evolved in kJ, during this combustion. (ΔH_c(CH₄)= - 890 kJ mol^-1 and (ΔH_c(C₂H₄) = -1423 kJ mol^-1

Write down the Born-Haber cycle for the formation of CaCl₂

Explain how heat absorbed at constant volume is measured using bomb calorimeter with a neat diagram.

Derive the relation between ΔH and ΔU for an ideal gas. Explain each term involved in the equation.

List the characteristics of Gibbs free energy

Calculate the entropy change in the system, and surroundings, and the total entropy change in the universe during a process in which 245 J of heat flow out of the system at 77°C to the surrounding at 33°C.

1 mol of PCl₅, kept in a closed container of volume 1 dm³ and was allowed to attain equilibrium at 423 K. Calculate the equilibrium composition of reaction mixture. (The K_c value for PCl₅ dissociation at 423 K is 2)

1 mol of CH₄, 1 mole of CS₂ and 2 mol of H₂S are 2 mol of H₂ are mixed in a 500 ml flask. The equilibrium constant for the reaction K_C = 4 x 10^–2 mol² lit^–2. In which direction will the reaction proceed to reach equilibrium ?

28 g of Nitrogen and 6 g of hydrogen were mixed in a 1 litre closed container. At equilibrium 17 g NH₃ was produced. Calculate the weight of nitrogen, hydrogen at equilibrium.

A sealed container was filled with 1 mol of A₂ (g), 1 mol B₂ (g) at 800 K and total pressure 1.00 bar. Calculate the amounts of the components in the mixture at equilibrium given that K = 1 for the reaction
A₂ (g) + B₂ (g) ⇌ 2AB (g)

The partial pressure of carbon dioxide in the reaction
CaCO₃ (s) ⇌ CaO (s) + CO₂(g) is 1.017 × 10^–3 atm at 500⁰C. Calculate K_p at 600⁰C for the reaction. ΔH for the reaction is 181 KJ mol^–1 and does not change in the given range of temperature.

Consider the following reaction
Fe³⁺(aq) + SCN^–(aq) ⇌ [Fe(SCN)]²⁺(aq)
A solution is made with initial Fe³⁺, SCN^- concentration of 1 x 10^-3 M and 8 x 10^-4 M respectively. At equilibrium [Fe(SCN)]²⁺ concentration is 2 x 10^-4 M. Calculate the value of equilibrium constant.

The following water gas shift reaction is an important industrial process for the production of hydrogen gas.
CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g)
At a given temperature K_p = 2.7. If 0.13 mol of CO, 0.56 mol of water, 0.78 mol of CO₂ and 0.28 mol of H₂ are introduced into a 2 L flask, and find out in which direction must the reaction proceed to reach equilibrium

The equilibrium constant for the following reaction is 0.15 at 298 K and 1 atm pressure.
N₂O₄(g) ⇌ 2NO₂(g);
\(\Delta \mathrm{H}_{\mathrm{f}}^{\circ}=57.32 \mathrm{KJmol}^{-1}\)
The reaction conditions are altered as follows.
a) The reaction temperature is altered to 100^o C keeping the pressure at 1 atm, Calculate the equilibrium constant.

At particular temperature K_C = 4 x 10^–2 for the reaction
H₂S(g) ⇌ H₂(g) + ½ S₂(g)
Calculate KC for each of the following reaction
i) 2H₂S (g) ⇌ 2H₂ (g) + S₂ (g)
ii) 3H₂S (g) ⇌ 3H₂ (g) + 3/2 S₂(g)

The equilibrium for the dissociation of XY₂ is given as,
2XY₂ (g) ⇌ 2XY (g) + Y₂(g)
if the degree of dissociation x is so small compared to one. Show that 2 K_P = PX₃ where P is the total pressure and K_P is the dissociation equilibrium constant of XY₂.

Calculate the proportion of O₂ and N₂ dissolved in water at 298 K. When air containing 20% O₂ and 80% N₂ by volume is in equilibrium with it at 1 atm pressure. Henry’s law constants for two gases are K_H(O₂) = 4.6 x 10⁴ atm and K_H (N₂) = 8.5 x 10⁴ atm.

Calculate the mole fractions of benzene and naphthalene in the vapour phase when an ideal liquid solution is formed by mixing 128 g of naphthalene with 39 g of benzene. It is given that the vapour pressure of pure benzene is 50.71 mm Hg and the vapour pressure of pure naphthalene is 32.06 mmHg at 300 K.

2.56 g of Sulphur is dissolved in 100g of carbon disulphide. The solution boils at 319. 692 K. What is the molecular formula of Sulphur in solution The boiling point of CS₂ is 319. 450K. Given that K_b for CS₂ = 2.42 K Kg mol^-1.

Henry’s law constant for solubility of methane in benzene is 4.2 x 10^-5 mm Hg at a particular constant temperature At this temperature.
Calculate the solubility of methane at
i) 750 mm Hg
ii) 840 mm Hg

The vapour pressure of pure benzene (C₆H₆) at a given temperature is 640 mm Hg. 2.2 g of non-volatile solute is added to 40 g of benzene. The vapour pressure of the solution is 600 mm Hg. Calculate the molar mass of the solute ?

0.26g of an organic compound gave 0.039 g of water and 0.245 g of carbon dioxide on combustion. Calculate the percentage of C & H.

0.2346g of an organic compound containing C, H & O, on combustion gives 0.2754g of H₂O and 0.4488g CO₂. Calculate the % composition of C, H & O in the organic compound [C = 52.17, H = 13.04, O = 34.79]

0.185 g of an organic compound when treated with Conc. HNO₃ and silver nitrate gave 0.320 g of silver bromide. Calculate the % of bromine in the compound. (Ag =108, Br = 80)

Give the IUPAC names of the following compounds.
(CH₃)₂CH – CH₂ – CH(CH₃) – CH(CH₃)₂

Give the structure for the following compound.
3- ethyl - 2 methyl -1-pentene

Elucidate the steps involved in arriving at the molecular formula of a compound.

Calculate the molecular mass of the following KMnO₄

Calculate the molecular mass of the following Crystalline oxalic acid

Calculate the molecular mass of the following Methane

Calculate the oxidation number of underlined atoms \(H_{ 4 }\underline { { P }_{ 2 } } { O }_{ 7 }\)

Mention the standards prescribed by BIS for quality of drinking water.

How does classical smog differ from photochemical smog ?

What are particulate pollutants ? Explain any three.

Ethane burns completely in air to give CO₂, while in a limited supply of air gives CO. The same gases are found in automobile exhaust. Both CO and CO₂ are atmospheric pollutants
i) What is the danger associated with these gases
ii) How do the pollutants affect the human body ?

How is acid rain formed ? Explain its effect

What is meant by nodal surface or node?

What is shape of the orbital with 
(i) n = 2 and = 0
(ii) n = 2 and I = 1?

Write the values of I and m for p-orbitals

Which quantum accounts for the orientation of the electron orbital?

Which energy level does not have p-orbital?

Assertion: Two mole of glucose contains 12.044 x 10²³ molecules of glucose
Reason: Total number of entities present in one mole of any substance is equal to 6.02 x 10²²
(a) both assertion and reason are true and the reason is the correct explanation of assertion
(b) both assertion and reason are true but reason is not the correct explanation of assertion
(c) assertion is true but reason is false
(d) both assertion and reason are false

According to the Bohr Theory, which of the following transitions in the hydrogen atom will give rise to the least energetic photon?

Which of the following elements will have the highest electro negativity ____________

Ionic hydrides are formed by _____________

RbO₂ is _____________

Write note on the necessity for Hund's rule.

Discuss the filling of electron in a carbon atom

Using angular distribution function discuss the shapes of s orbitals

Explain the shapes of p orbitals

Discuss the shapes of d orbitals.

Name the third chalcogen and fifth noble gas

Lanthanoids and actinoids are placed in separate rows at the bottom of the periodic table. Explain.

Helium has a electronic configuration of 1s² but placed in p block in group 18. Justify.

Describe in brief Lothar Meyer's classification of elements.

Explain classification of elements based on Newland's law of Octaves.

Which one of the following represents 180 g of water ?

If n = 6, the correct sequence for filling of electrons will be __________

The electronic configuration of the atom having maximum difference in first and second ionisation energies is _________

In case of alkali metal halides, the ionic character increases in the order ____________

The value of universal gas constant depends upon __________

Which of the following species will have the largest and smallest size Mg, Mg²⁺, AI, Al³⁺? Give reason.

The size of Cl^- = 1.81Å and CI = O.99Å. Explain.

How does the shielding effect caused by inner electrons affect the ionisation energy?

Larger the size of the atom, lesser is the ionisation energy. Explain.

Define Ionization enthalpy.

Explain the laboratory preparation of dihyodrogen.

Why is water molecule polar?

Distinguish between (i) hard water and soft water 

Distinguish between (ii) temporary hardness and permanent hardness.

(i) Can marine species live in distilled water?
(ii) Can distilled water be called as deionised water?

What do you understand by the term mole ?

How many orbitals are possible for n = 4?

Is the definition given below for ionisation enthalpy correct?
"Ionisation enthalpy is defined as the energy required to remove the most loosely bound electron from the valence shell of an atom.

Predict which of the following hydrides is a gas on a solid
(a) BCI
(b) NaH 
Give your reason.

Substantiate lithium fluoride has the lowest solubility among group one metal fluorides.

Mention any two biological effects of D₂O.

Name the salts that lead to the formation of permanent hardness in water can you remove permanent hardness by boiling?

How will you regenerate zeolite in ion-exchange method?

What kind of compounds can be dissolved and hydrolysed in water?

Water is a useful solvent. Which properties make water as a good solvent?

Which contains the greatest number of moles of oxygen atoms
i) 1 mol of ethanol
ii) 1 mol of formic acid
iii) 1 mol of H₂O

An atom of an element contains 35 electrons and 45 neutrons. Deduce
(i) the number of protons
(ii) the electronic configuration for the element
(iii) All the four quantum numbers for the last electron

How would you explain the fact that the second ionisation potential is always higher than first ionisation potential?

NH₃ has exceptionally high melting point and boiling point as compared to those of the hydrides of the remaining element of group 15. Explain.

How is plaster of paris prepared ?

Lithium salts are more soluble than the salts of other metals of group 1. Justify.

How does the alkali metals produce characteristic colour to the oxidising flame

Why is the density of potassium less than that of sodium?

Why are potassium and caesium, rather than lithium used in photochemical cells?

Why does lithium exhibit anomalous properties?

How many moles of ethane is required to produce 44 g of CO_2(g) after combustion.

The electronic configuration of atom is one of the important factor which affects the value of ionisation potential and electron gain enthalpy. Explain.

Complete the following chemical reactions and classify them into
(a) hydrolysis (b) redox (c) hydration reactions.
(1) KMnO₄ + H₂O₂ ➝
(2) CrCl₃ + H₂O ➝
(3) CaO + H₂O ➝

Write balanced chemical equation for each of the following chemical reactions.
Lithium metal with nitrogen gas.

What are ideal gases? In what way real gases differ from ideal gases.

List the uses of sodium hydroxide

Why is sodium bicarbonate nicknamed as 'Baking Soda'?

Give the uses of sodium bicarbonate

Why table salt becomes wet when kept in open space?

Why does Li₂CO₃ decompose at a temperature below 1273K?

What is the difference between molecular mass and molar mass ? Calculate the molecular mass and molar mass for carbon monoxide.

Describe the Aufbau principle

Justify that the fifth period of the periodic table should have 18 elements on the basis of quantum numbers.

What is water-gas shift reaction?

Give the systematic names for the following
Milk of magnesia

What is compressibility factor? How does it explain the deviation of non ideal gases from ideal behaviour.

Explain the term 'Boyle's point.' Mention is significance.

Show how the molar volume of a real and ideal gas are related to each other?

Using Andrew's isotherm of CO₂ explain the terms
(i) critical temperature
(ii) critical pressure and
(iii) critical volume.

What is inversion temperature? How is it related to Vander Waals constants?

A Compound on analysis gave Na = 14.31% S = 9.97% H = 6.22% and 0 = 69.5%.
Calculate the molecular formula of the compound if all the hydrogen in the compound is present in combination with oxygen as a water of crystallization. (molecular mass of the compound is 322).

What is the de Broglie wave length of an electron, which is accelerated from the rest, through a potential difference of 100 V ?

What is screening effect? Briefly give the basis for pauling's scale of electronegativity.

A group-1 metal (A) which is present in common salt reacts with (B) to give compound (C) in which hydrogen is present in –1 oxidation state. (B) on reaction with a gas (C) to give universal solvent (D). The compound (D) on reacts with (A) to give (E), a strong base. Identify A, B, C, D and E. Explain the reactions.

Describe briefly the biological Importance of Calcium and magnesium.

Write the Consequence of Boyle's law.

Explain Charles' law with an experimental illustration.

Explain the graphical representation of Charles law.

Explain graphical representation of Gay Lussac's law.

Explain the graphical representation of Avogadro's hypothesis.

Calculate the percentage composition of the elements present in magnesium carbonate. How many kilogram of CO₂ can be obtained by heating 1 kg of 90 % pure magnesium carbonate.

What is the de Broglie wave length of an electron, which is accelerated from the rest, through a potential difference of 100 V ?

Why the first ionisation enthalpy of sodium is lower than that of magnesium while its second ionisation enthalpy is higher than that of magnesium.

Explain preparation of hydrogen using electrolysis.

Describe briefly the biological Importance of Calcium and magnesium.

For a reaction, 2Cl_(g) ⟶ Cl₂, What are the signs of ΔH and ΔS?

In the equation N_2(g)+ 3H_2(g) ⇌2NH_3(g) What would be the sign of work done?

Which law of thermodynamics deals with equivalence of different forms of energies?

Define the following terms.

Define the term thermodynamic process.

Define entropy of fusion.

Define entropy of vapourisation.

Define entropy of transition.

What are spontaneous process?

What is absolute zero temperature?

What happens when the' concentration of H₂ and I₂ are increased in the reaction \({ H }_{ 2 }+{ I }_{ 2 }\rightleftharpoons 2HI?\)

Discuss the changes you observe in the reaction of I synthesis of ammonia with preference to effect of pressure.

Write a note on Haber's process emphasizing the idea of effect of a catalyst in an equilibrium reaction.

What inferences do you observe by the values of Q andK_c?

Explain about th formation of solid-liquid equilibrium with suitable example.

Explain the effect of concentration of reactants on an equilibrium with example

Consider the reaction, N₂(g) + 3H₂(g) ⇌ 2NH₃(g). Explain the effect of pressure on this equilibrium reaction.

Why pressure has no effect on the synthesis of HI?

Explain the effect of temperature on the following equilibrium reaction.
N₂(g) + 3H₂Cg)⇌ 2NH₃(g)Δ H = - 92.2 kJ.

How does oxygen exchanges between maternal and fetal blood in a pregnant women ?

Enlist the advantages using standard solutions.

Write a note on solubility of solute and brief out the formation of a saturated solution with an example.

Explain the above variation in solubility with respect to temperature for selective compounds.

With the help of a graph discuss the variation of vapour pressure of benzene in toluene.

Discuss the comparison between Raoult's law and Henry's law.

What are gaseous solution ? Give its various types with example.

What are liquid solutions ? Explain with example.

What are solid solution ? Give example.

How will you prepare a standard solution ?

What are the advantages of standard solution.

Draw the lewis structure of
(i) Ammonia
(ii) Methane
(iil) Dinitrogen pentoxide.

Calculate the bond enthalpy of OH bond in water.

Explain how the ionic character in a covalent bond is related to electronegativity?

CuCI is more covalent than NaCl. Give reason.

Explain the bonding in oxygen molecule.

Distinguish between a sigma bond and a pi bond.

Write the important conditions required for the linear combination of atomic orbitals to form molecular orbitals.

What are Lewis structures? Write the Lewis structure of H₂, BeF₂ and H₂O.

What are the main postulates of Valence Shell Electron Pair Repulsion (VSEPR) theory ?

Explain why BeH₂ molecule has a zero dipole moment although the Be - H bonds are polar.

What is the difference between distillation, distillation under reduced pressure and steam distillation?

How will you derive the molecular structure from the type of hybridisation?

Define the term isomerism and write a short note on its classification.

Write a short note on homologous series.

Write a note on cis-trans isomerism in oximes and azo compounds.

Discuss the conditions for optical isomerism.

How would you detect the presence of carbon and hydrogen in a compound?

(i) Give the test to predict the .presence of Cl, Br and I in an organic compound.
(ii) How will you eliminate in Nand S present in an organic halogen compund?

Explain how benzoic acid (or Naphthalene or camphor) purified. (or) Explain how a substance is purified by sublimation.

Suggest and explain the method suitable to purify the organic compounds depending on their boiling points.

While writing the resonance structures, what are the rules to be followed ?

Distinguish between electrophiles and nucleophiles

Illustrate with examples, the three types of electron movement in organic reaction.

Discuss the reason behind the classification of inductive effect into +I and -I effect.

Explain the different types of substitution reactions or displacement reactions.

Carry over the following reaction mechanisms.
(i) Bromination of alkene
(ii) Addition of HCN to CH₃CHO
(iii) Formation of alkyl bromide with benzoyl peroxide as radical initiator.

Which of the following compounds will not exist as resonance hybrid? Give reason for your answer.
(i) CH₃ - OH
(ii) R-CONH₂
(iii) CH₃-CH = CH-CH₂NH₂

Which bond is more polar in the following pair of molecular?
(i) H₃C-H (or) H₃C-Br
(ii) H₃C-NH₂ (or) H₃C-OH
(iii) H₃C-OH (or) H₃C-SH

Write structures of various carbocations that can be obtained from 2-methyl butane. Arrange these carbocations in order of increasing stability.

The structure of triphenylmethyl cation is given below. This very stable and some of its salts can be stored for months. Explain the cause of high stability of this cation.

Write a brief note on polymerisation of alkenes.

How many types of polymerisation are possible in alkynes?

State Huckel's rule of aromaticity and explain it interms of cyclopentadiene, cycloxtateraene and cyclopropenylcation.

Among anthracene and cyclopentadiene which is aromatic? Give reason for your answer.

Explain the molecular orbirtal structure of benzene.

Explain the polymerisation of acetylene. write notes on
i) Linear polymerisation ii) Cyclic polymerisation

Discuss the Kekule's structure of benzene.

Why benzene undergoes substitution reaction rather than addition reactions under normal conditions?

Explain the industrial preparation of benzene from coal tar.

Explain the sulphonation of benzene.

Explain the hydrolysis of 2-bromobutane with aqueous KOH.

Explain the action of alcoholic KOH with 2-bromobutane.

Mention the uses of chloroform

What are the uses of carbon tetrachloride?

What are ogranometallic compounds? Give one example: Explain the nature of the carbon-metal bond.

What are the uses of freons?

What is DDT? How is it prepared?

Mention the uses of DDT.

Write the equations for the preparation of l-iodobutane from.

Explain why:
(i) the dipole moment of chlorobenzene is lower than that of cyclohexyl chloride?
(ii) alkyl halides though polar, are immiscible with water?
(iii) Gringard reagents should be prepared under anhydrous conditions?

Explain how hydrocarbons pollute the atmospheric air.

Write notes about great London smog.

What are the effects of classical smog ?

Explain how oxides of nitrogen are introduced directly into the stratosphere?

How chemical wastes pollute water?

Explain how styrene is produced by traditional and greener routes ?

How acetaldehyde is commercially prepared by green chemistry?

What do you mean by ozone hole? What are its consequences?

What is photochemical smog? What are its effects ? How can it be controlled ?

(a) Define eutrophication and pneumoconiosis.
(b) Write differences between photochemical smog and classical smog

What is environmental pollution ? How is it caused ?

Discuss in detail about the gaseous air pollutants.

What is acid rain ? How is caused ? Enlist its harmful effects ?

What are non-viable particulates ? How are they classified ? Explain.

Discuss the health hazards caused by particulate pollutants.

List out some methods that you suggest to control water pollution in your locality.

Explain about the different layers of Earth's atmosphere.

What are the health effects of particulate pollutants?

What are the effects of photochemical smog?

Explain about the environmental impacts of ozone depletion.

Explain the classification of organic compounds with example.

Explain SN₂ mechanism with suitable examples.

SN₂ reaction of an optically active haloalkane is accompanied by inversion of configuration at the asymmetric centre. Prove it.

Explain E₂ reaction mechanism with a suitable example.

Describe E₁ reaction mechanism with a suitable example

The simplest aromatic hydrocarbon C₆H₆ reactsⒷ on treatment with sodium hydroxide will (C₆H₅OH), Phenol, © as the product. Also Cl₂ to giveⒶ which on reaction with sodium hydroxide gives Ⓑ.Ⓑ of molecular formula C₆H₆O. @ on treatment with ammonia will give C₆H₇N as @. Identify Ⓐ, Ⓑ, ©, and explain the reactions involved.

An organic compound Ⓐ of molecular formula C₂H₂ reacts with HCI to give C₂ H₄Cl₂ asⒷ.Ⓑon reaction with aqueous KOH will give C₂H₄Oas Ⓒ Identify Ⓐ,Ⓑ, © and explain the reactions involved.

Two isomers of formula C₄H₉ Br are Ⓐ and B, Ⓐ on reaction with alcoholic KOH gives of molecular formula C₄H₈by E₁ reaction. .Ⓑ on reaction with alcoholic KOH gives Ⓓ and Ⓔ as products by Saytzeff's rule. Identify A, B, C, D, E

A simple aromatic hydrocarbon Ⓐ reacts with Cl₂ to give @ of molecular formula C₆H₅Cl.Ⓑ on reaction with ethyl chloride along with sodium metal gives © of formula C₈H₁₀. © alone reacts with Na metal in the presence of ether to give © C₁₂H₁₀. Identify Ⓐ, Ⓑ, © & Ⓓ

An organic compound Ⓐ of molecular formula CH₂O reacts with methyl magnesium iodide followed by acid hydrolysis to give Ⓑ of molecular formula C₂H₆0. Ⓑ on reaction with PCIs gives ©. ©on reaction with alcoholic KOH gives Ⓓan alkene as the product. Identify Ⓐ, Ⓑ ©, Ⓓ and explain the reactions involved.

Explain various methods of preparation of alkane.

Discuss in detail about the conformations exhibited by ethane.

How are alkene's obtained by Kolbe's electrolytic method (or) How will you Prepare ethene fro Potassium succinate?

How is the structure of benzene elucidated?

Explain in detail about the addition of hydrogen halide to an unsymmetrical alkene.

Explain the acidic nature of alkynes.

Write the mechanism of chlorination of benzene.

Describe the mechanism of sulphonation of benzene.

Describe the mechanism of Freidel craft's alkylation.

Write the mechanism of Freidel craft's acylation

Explain electron movement in organic reactions.

How does inductive effect influence the reactivity and acidity of carboxylic acids ?

How is resonance useful in explaining the acidity of phenol ?

How does hyper conjugation effect explain the stability of alkenes ?

Explain the types of addition reactions ?

Explain the types of substitution reaction ?

For the following bond cleavages use curved-arrows to show the electron flow and classify each as homolytic or heterolytic fission. Identify reactive intermediate produced as free radical, carbocation and carbanion ?
(a) \({ CH }_{ 3 }O-O{ CH }_{ 3 }\longrightarrow { CH }_{ 3 }\overset { \bullet }{ O } +{ CH }_{ 3 }\overset { \bullet }{ O } \) 
(b)

(c)

(d)

An organic compound (A) has a molecular formula C₂H₆0 it is one of the primary alcohol. A reacts with acidified potassium dichromate to give B. B on further undergoes to oxidation reaction to give C. C on reacts with SOCl₂ to give D which is chlorinated product. Identify A,B,C and D, explain with equation.

An organic compound (A) of a molecular formula C₂H₄ which is a simple alkene. A reacts with dil H₂SO₄ to give B. A again reacts with Cl₂ to give C. Identify A,B and C and write the equations.

Complete the reactions and identify the products.
(i)

(ii)
\({ CH }_{ 3 }-\underset { \overset { | }{ Cl } }{ C } H-{ CH }_{ 3 }\overset { { H }^{ + }/{ K }_{ 2 }{ Cr }_{ 2 }{ O }_{ 7 } }{ \longrightarrow } A\overset { (O)) }{ \longrightarrow } B\)

List down the characteristics possessed by the organic compounds.

Explain the following with example.
(i) Fisher projection formula
(ii) Saw horse projection formula
(iii) Newman projection formula

Describe tautomerism with relevant examples.

How would you estimate the percentage of carbon and hydrogen in an organic compound?

How would you estimate the percentage of sulphur in an organic compound by Carius method?

Explain about lassaigne's test for detection of nitrogen in an organic compound.

Explain about the estimation of carbon and hydrogen.

Explain about the estimation of halogens by carius method.

How will you estimate phosphorous in an organic compound?

Explain Dumas method of estimation of nitrogen.

40 ml of methane is completely burnt using 80 ml of oxygen at room temperature The volume of gas left after cooling to room temperature is _______.

Assertion: Two mole of glucose contains 12.044 x 10²³ molecules of glucose
Reason: Total number of entities present in one mole of any substance is equal to 6.02 x 10²²
(a) both assertion and reason are true and the reason is the correct explanation of assertion
(b) both assertion and reason are true but reason is not the correct explanation of assertion
(c) assertion is true but reason is false
(d) both assertion and reason are false

The equivalent mass of a trivalent metal element is 9 g eq^-1 the molar mass of its an hydrous oxide is _____.

1 g of an impure sample of magnesium carbonate (containing no thermally decomposable impurities) on complete thermal decomposition gave 0.44 g of carbon dioxide gas. The percentage of impurity in the sample is ______________.

When 22.4 litres of H₂(g) is mixed with 11.2 litres of Cl₂(g), each at 273 K at 1 atm the moles of HCl (g), formed is equal to ______.

Write note on combination reaction.

Write note on decomposition reaction

Explain displacement reaction ? Explain its two types with an example for each.

What are disproportionation reaction (or) auto redox reactions ? Give examples.

Arrange the elements silver, Zinc and copper in the order of their decreasing electron releasing tendency and justify your arrangement with an appropriate experiment.

The equivalent mass of ferrous oxalate is __________.

Two 22.4 litre containers A and B contains 8 g of O₂ and 8 g of SO₂ respectively at 273 K and 1 atm pressure, then ______.

The mass of a gas that occupies a volume of 612.5 ml at room temperature and pressure (25⁰ c and 1 atm pressure) is 1.1g. The molar mass of the gas is _______.

Which of the following compound(s) has /have a percentage of carbon same as that in ethylene (C₂H₄)?

Which one of the following is used as a standard for atomic mass?

Balance the following equations by oxidation number method.
Zn + HNO₃ ⟶ Zn(NO₃)₂ + N₂O + H₂O

Balance the following equations by oxidation number method.
Ag + HNO₃ ⟶ AgNO₃ + H₂O + NO

Balance the following equations by oxidation number method.
K₂Cr₂O₇ + FeSO₄ + H₂SO₄ ⟶ K₂SO₄ + Cr₂(SO₄)₃ + Fe₂(SO₄)₃ + H₂O

Balance the following equations by oxidation number method.
KBr + MnO₂ + H₂SO4 ⟶ KHSO₄ + MnSO₄ + H₂O + Br₂

Balance the following equations by oxidation number method.
KMnO₄ + KOH + H₂O₂ ⟶ K₂MnO₄ + O₂ + H₂O

If n = 6, the correct sequence for filling of electrons will be __________

How many electrons in an atom with atomic number 105 can have (n + 1) = 8 ? 

If uncertainty in position and momentum are equal, then minimum uncertainty in velocity is _________

The ratio of de Broglie wavelengths of a deuterium atom to that of an \(\alpha\) - particle, when the velocity of the former is five times greater than that of later, is ____________

Time independent Schnodinger wave equation is ______________

Enlist the postulates of Bohr's atom model.

By applying Bohr's postulates, arrive at the radius of n^th orbit for hydrogen like atom

Write a note on limitations of Bohr's atom model.

Derive an equation for the wavelength of a matter wave.

List out the important features of quantum mechanical model of atom

The energy of light of wavelength 45 nm is _____________.

Splitting of spectral lines in an electric field is called _____________

Which of the following pairs of d-orbitals will have electron density along the axes ?

Two electrons occupying the same orbital are distinguished by ___________

For d-electron, the orbital angular momentum is ___________

Calculate the de-Broglie wavelength of an electron that has been accelerated from rest through a potential difference of 1 keV.

Calculate the uncertainty in the position of an electron, if the uncertainty in its velocity is 5.7 x 10⁵ ms^-1.

Calculate the total number of angular nodes and radial nodes present in 3d and 4f orbitals.

Explain about
(i) Magnetic quantum number
(ii) Spin quantum number

Explain the angular distribution function of 1s, 2s, 3s, 2p, 3d and 4f orbits.

The electronic configuration of the atom having maximum difference in first and second ionisation energies is _________

IE₁ and IE₂ of Mg are 179 and 348 kcal mol^-1 respectively. The energy required for the reaction Mg⟶ Mg²⁺ + 2e^- is ___________

Which of the following orders of ionic radii is correct?

Which one of the following is true about metallic character when we move from left to right in a period and top to bottom in a group?

Which of the following pairs of elements exhibit diagonal relationship?

Give the structural features of modern periodic law.

Mention Anomalies of Mendeleev's periodic table.

How do you classify of elements into blocks? Give their electronic configuration.

Give the characteristics of p-block elements.

Give any five characteristic properties of inner transition elements.

The electronic configuration of the elements A and B are 1s², 2s ²,2p⁶,3s² and 1s², 2s²,2p⁵ respectively. The formula of the ionic compound that can be formed between these elements is ___________

In which of the following options the order of arrangement does not agree with the variation of property indicated against it?

Various successive ionisation enthalpies (in kJ mol^-1) of an element are given below.

The element is

Identify the wrong statement.

The correct order of electron gain enthalpy with negative sign of F, Cl, Br and I having atomic number 9, 17, 35 and 53 respectively is _____________

Explain about the anomalies of Mendeleev's periodic table.

Explain about the structural features of Moseley's long form of periodic table.

Explain the merits of Moseley's long form of periodic table.

Explain about the general characteristics of periods.

Explain about the salient features of groups.

For decolorisation of 1 mole of acidified KMnO₄, the moles of H₂O₂ required is ___________

The hybridisation of oxygen atom is H₂O and H₂O₂ are, respectively __________

In solid ice, oxygen atom is surrounded _____________

Heavy water is used as _________

Assertion: Permanent hardness of water is removed by treatment with washing soda.
Reason: Washing soda reacts with soluble calcium and magnesium chlorides and sulphates in hard water to form insoluble carbonates

Why hard water is not suitable for laundry ?

Explain the laboratory preparation of hydrogen.

Explain the action of water on
1) Na
2) Ba
3) Fe
4) Pb & Cu
5) Ag, Au,& Hg & Pt
6) C, S, & P

Give the chemical properties of heavy water and water.

Calculate
(i) Concentration of H₂O₂ in g/L 
(ii) Normally

Water gas is _____________

Ionic hydrides are formed by _____________

Non-stoichiometric hydrides are formed by _____________

The hardness of water can be determined by volumetrically using the reagent _____________

Zeolite used to soften hardness of water is hydrated _____________

Explain about Hydrogen sponge

How are reducing agents in synthetic organic chemistry prepared?

How does water react with
(i) SiCI₄
(ii) P₄O₁₀

Explain about the structure of CuSO₄.5H₂O

How is hydrogen peroxide prepared on industrial scale?

In context with beryllium, which one of the following statements is incorrect ?

A colourless solid substance (A) on heating evolved CO₂ and also gave a white residue, soluble in water. Residue also gave CO₂ when treated with dilute HCI ___________

Which of the following statement is false ?

Formula of Gypsum is _______________

Among the following the least thermally stable is ___________

List out the uses of alkali metals

How are peroxides and superoxides formed by alkali metals?

The hydrides of alkali metals behave as strong reducing agents - Justify the statement.

When does the blue coloured ammonia solution (of alkali metals) changes to bronze colour?

Bring out the simularities between lithium and magnesium.

Which of the following compounds will not evolve H₂ gas on reaction with alkali metals ?

sodium is stored in _____________

Find the wrong statement

In case of alkali metal halides, the ionic character increases in the order ____________

The product obtained as a result of a reaction of nitrogen with CaC₂ is ___________

Illustrate the role of sodium and potassium in biological fluid

How is sodium hydroxide prepared commercially from brine solution?

Compare the properties of beryllium with other elements of the same group.

Explain the preparation and uses of the following compounds of calcium.

When water is added to compound (A) of calcium, compound B is formed with a hissing sound and evolution of large amount of heat. When CO₂ is passed into the solution, it turns milky due to the formation of compound C. If excess CO₂ is passed into the solution, milkiness disappears due to the formation of compound (D). Identify the compounds A, B, C and D. Explain why the milkiness disappears in the last step.

A bottle of ammonia and a bottle of HCI connected through a long tube are opened simultaneously at both ends. The white ammonium chloride ring first formed will be ___________

The value of the gas constant R is ____________

The table indicates the value of van der Waals constant 'a' in (dm³)² atm. mol^-2.

The gas which can be most easily liquefied is ______________

If temperature and volume of an ideal gas is increased to twice its values, the initial pressure P becomes _________

The variation of volume V, with temperature T, keeping pressure constant is called the coefficient of thermal expansion ie \(\alpha =\frac { 1 }{ V } { \left( \frac { \partial V }{ \partial T } \right) }_{ P }\) For an ideal gas a is equal to ___________

Explain P-V relationship experiments of Robert Boyle.

Derive the ideal gas equation by combining the empirical gas laws.

Using the ideal gas equation how will you calculate the values of R ?

Defined the following terms.

Explain Andrew's isotherm.

The variation of volume V, with temperature T, keeping pressure constant is called the coefficient of thermal expansion ie \(\alpha =\frac { 1 }{ V } { \left( \frac { \partial V }{ \partial T } \right) }_{ P }\) For an ideal gas a is equal to ___________

Maximum deviation from ideal gas is expected from ______________

Assertion: Critical temperature of CO₂ is 304K, it can be liquefied above 304K.
Reason : For a given mass of gas, volume is to directly proportional to pressure at constant temperature

Which of the following diagrams correctly describes the behaviour of a fixed mass of an ideal gas? (T is measured in K)

In a closed room of 1000 m³ a perfume bottle is opened up. The room develops smell. This is due to which property of gases _____________

The van der waal's constant 'b' for oxygen is 0.0318 L mol^-1. Calculate the diameter of the oxygen molecule.

An LPG cylinder containing 15 kg of butane at 27° C and 10 atmpressure is leaking. After one day, its pressure is decreased to 8 atm. How much quality of the gas is leaked ?

Arrive at the values of gas constant (R) in dm³ atm mol^-1 K^-1, Pa, m³ K^-1, mol^-1 at JK^-1 mol^-1.

Explain Andrew's isotherm of carbon dioxide.

Express mathematically Dalton's law of partial pressures.

The amount of heat exchanged with surrounding at constant temperature pressure is given by the quantity ______________

In an adiabatic process, which of the following is true ?

In a reversible process, the change in entropy of the universe is ________________

In an adiabatic expansion of an ideal gas ____________

The intensive property among the quantities below is ____________

If an automobile engine burns petrol at a temperature of 816° C and if the surrounding temperature is 21° C, calculate its maximum possible efficiency

Calculate the entropy change in the engine that receives 957.5 kJ of heat reversibly at 110°C temperature.

Calculate the standard entropy change for the following reaction (Δs_f⁰), given the standard entropies of CO_2(g) ,  C_(s) 'O_2(g) as 213.6, 5.740, and 205 JK^-1 respectively.

Calculate the entropy change during the melting of one mole of ice into water at 0°C and 1 atm pressure. Enthalpy of fusion of ice is 6008 J mol^-1.

The entropy change in the conversion of water to ice at 272 k for the system is -22.88 Jk^-1mol^-1 and that of surrounding is + 24.85 Jk^-1 mol-¹, State whether the process is spontaneous or not?

All the naturally occurring processes proceed spontaneously in a direction which leads to _______________

In a reversible process, the change in entropy of the universe is ________________

In an adiabatic expansion of an ideal gas ____________

The intensive property among the quantities below is ____________

An ideal gas expands from the volume of 1 x 10^-3 m³ to 1 x 10^-2 m³ at 300 K against a constant pressure at 1 x 10⁵ Nm^-2. The work done is ______________

Discuss in detail about the variation of internal energy with respect to various thermodynamic processes

Write down the conventions that are followed while framing a thermo chemical equation

Explain the measurement of heat change at constant pressure with a neat diagram.

The enthalpy of combustion for H₂, C_(graphite) and CH₄ are -285.8, -393.5 and -890.4 kJ mol^-1respectively. Calculate the standard enthalpy of formation \(\Delta { H }_{ f }^{ 0 }\) for CH₄

Calculate the lattice energy of MgBr₂ from the given data

\({K_c\over K_p}\) for the reaction,
N₂(g) + 3H₂(g) ⇌ 2NH₃(g) is ___________

In which of the following equilibrium, K_P and K_C are not equal ?

If x is the fraction of PCl₅ dissociated at equilibrium in the reaction
PCl₅ ⇌ PCl₃ + Cl₂
then starting with 0.5 mole of PCl₅, the total number of moles of reactants and products at equilibrium is ___________

The values of K_P1 and K_P2 for the reactions
X ⇌ Y + Z
A ⇌ 2B are in the ratio 9 : 1 if degree of dissociation and initial concentration of X and A be equal then total pressure at equilibrium P₁ and P₂ are in the ratio __________

In the reaction,
Fe (OH)₃ (s) ⇌ Fe³⁺(aq) + 3OH^–(aq),
if the concentration of OH^– ions is decreased by ¼ times, then the equilibrium concentration of Fe³⁺ will

Explain: How does the extent of reaction depend on K_c?

PCI₅ PCl₃ and Cl₂ are at equilibrium at 500 K and having concentration 1.59M PCI₃ , 1.59M Cl₂ and 1.41M PCI_5. Calculate Kc for the reaction PCI₅ ⇌ PCl₃ + Cl_2.

Derive K_c and K_p expressions for the equilibrium: x_A+ y_B ⇌ lC+ mD

Derive the expressions for K_C and K_P, for the synthesis of Hl.

Derive the values of K_p and K_c for dissociation of PCl_5.

Which of the following is not a general characteristic of equilibrium involving physical process ___________

For the formation of Two moles of SO₃(g) from SO₂ and O₂, the equilibrium constant is K₁. The equilibrium constant for the dissociation of one mole of SO₃ into SO₂ and O₂ is __________

[Co(H₂O)₆]²⁺ (aq) (pink) + 4Cl^– (aq) ⇌ [CoCl₄]^2– (aq) (blue) + 6 H₂O (l)
In the above reaction at equilibrium, the reaction mixture is blue in colour at room temperature. On cooling this mixture, it becomes pink in colour. On the basis of this information, which one of the following is true?

The equilibrium constants of the following reactions are:

The equilibrium constant (K) for the reaction ;
\({ 2NH }_{ 3 }+5/2{ O }_{ 2 }\overset { K }{ \rightleftharpoons } 2NO+{ 3H }_{ 2 }{ O },\) will be

A 20 litre container at 400 K contains CO₂ (g) at pressure 0.4 atm and an excess of SrO (neglect the volume of solid SrO). The volume of the container is now decreased by moving the movable piston fitted in the container. The maximum volume of the container, when pressure of CO₂ attains its maximum value will be: Given that: SrCO₃ (S) ⇌ SrO (S) + CO₂(g)
KP = 1.6 atm

Derive the K_p and K_c for the following equilibrium reaction.
\({ H }_{ 2\left( g \right) }+{ I }_{ 2\left( g \right) }\rightleftharpoons { 2HI }_{ \left( g \right) }\)

Derive the expressions for K_c and K_p for the dissociation of PCI₅

(i) Describe the effect of
(a) addition of H₂,
(b) addition of CH₃0H
(c) removal of CO
(d) removal ofCH₃OH on the equilibrium of
the reaction, \({ 2H }_{ 2(g) }+{ CO }_{ (g) }\rightleftharpoons { CH }_{ 3 }{ OH }_{ (g) }\)
(ii) What happens to an equilibrium in a reversible reaction if a catalyst is added to it?

At certain temperature and under a pressure of 4 atm, PCl₅ is 10% dissociated. Calculate the pressure at which PCls will be 20% dissociated at temperature remaining constant.

What is the equilibrium concentration of each of the substances in the equilibrium when the initial concentration of ICI was 0.78 M?
2 ICI(g) ⇌ I₂(g) + Cl₂(g); K_C = 0.14

Two liquids X and Y on mixing gives a warm solution. The solution is __________

The relative lowering of vapour pressure of a sugar solution in water is 3.5\(\times\)10^–3. The mole fraction of water in that solution is ___________

For a solution, the plot of osmotic pressure (\(\pi\)) verses the concentration (c in mol L^–1) gives a straight line with slope 310R where 'R' is the gas constant. The temperature at which osmotic pressure measured is ____________

The Van't Hoff factor (i) for a dilute aqueous solution of the strong elecrolyte barium hydroxide is _____________

What is the molality of a 10% W/W aqueous sodium hydroxide solution ?

How does the change in temperature affect the solubility of a solute in a liquid solvent and gaseous solute in liquid solvent? Explain.

"Rate of vapourisation is reduced by presence of non-volatile solute"- Explain,

Explain the nature of non - ideal solution with positive deviation from Raoult,s law.

(i) When does a non-ideal solution is said to show a negative deviation?
(ii) Analyse the deviation observed in the solution of phenol and aniline.

Explain the various factors which are responsible for the deviation of solution from Raoult's law.

The molality of a solution containing 1.8g of glucose dissolved in 250 g of water is _____________

Which of the following concentration terms is/are independent of temperature _____________

Stomach acid, a dilute solution of HCl can be neutralised by reaction with Aluminium hydroxide
Al (OH)₃ + 3HCl (aq) → AlCl₃ + 3 H₂O
How many millilitres of 0.1 M Al(OH)₃ solution are needed to neutralise 21 mL of 0.1 M HCl ?

The Henry's law constant for the solubility of Nitrogen gas in water at 350 K is 8 x 10⁴ atm. The mole fraction of nitrogen in air is 0.5. The number of moles of Nitrogen from air dissolved in 10 moles of water at 350K and 4 atm pressure is ____________

Osometic pressure (p) of a solution is given by the relation ____________

Explain about the factors that are responsible for deviation from Raoult's law.

How will you obtain the molecular mass of a solute from relative lowering of vapour pressure ?

Derive an expression for molecular weight of the solute from osmotic Pressure.

What are ideal and non-ideal solutions ? Explain with suitable diagram the behaviour of ideal solutions.

Explain with a suitable diagram and appropriate example, why some non-ideal solution shows positive deviation from Raoult's

Xe F₂ is isostructural with _____________

According to VSEPR theory, the repulsion between different parts of electrons obey the order.

Non- Zero dipole moment is shown by __________

Among the following, the compound that contains, ionic, covalent and Coordinate linkage is ____________

The percentage of s-character of the hybrid orbitals in methane, ethane, ethene and ethyne are respectively ___________

Explain about valence bond theory for the formation of H₂ molecule.

What are the salient features of Valence Bond (VB) theory?

Explain about sp hybridisation with suitable example.

Draw the lewis structure for
Sulphur trioxide (SO₃)

Draw the lewis structure for
Phosphoric acid

In the molecule O_A = C = O_B, the formal charge on O_A, C and O_B are respectively.

Which of the following molecule contain no л bond ?

Which one of the following is the likely bond angles of sulphur tetrafluoride molecule ?

According to Valence bond theory, a bond between two atoms is formed when _____________

When one s and three p orbitals hybridise,

Explain about Kossel-Lewis approach to chemical bonding.

Explain about the salient features of molecular orbital theory.

Draw the M.OI. diagram of No molecule. Calculate its bond order and show that its paramagnetic.

Explain about metallic bonding

Explain about the bonding in metals by molecular orbital theory.

The IUPAC name of the compound \({ H }_{ 3 }C-\overset { \underset { | }{ { CH }_{ 3 } } }{ \underset { \overset { | }{ { CH }_{ 3 } } }{ C } } -CH=C{ \left( { CH }_{ 3 } \right) }_{ 2 }\) is _____________

The IUPAC name of the compound  \({ CH }_{ 3 }-\underset { \overset { | }{ OH } }{ CH } -COOH\) is _____________

The structure of isobutyl group in an organic compound is_______________________

Which of the following is optically active?

How many cyclic and acyclic isomers are possible for the molecular formula C₃H₆O?

Assertion : Fluorine has an oxidation state of - 1 in all its compounds.
Reason : Fluorine is the most electronegative element of the periodic table.

In Rutherford's gold foil experiment, a thin gold foil was bombarded with a stream of fast moving ___________

The statement that is not correct for modern classification of element is
(1) The properties of elements are periodic function of these atomic numbers.
(2) The ionisation enthalpy of the elements generally increase with increase in atomic number
(3) For transition elements the 3d orbitals are filled after 3p-orbitals and befire 4s orbitals.
(4) Fifth period contain 18 elements.

___________ torches is/are used in cutting and welding of a steel.

Half life of francium is _______

One 'U' stands for the mass of ______________.

Which of the following about the electron is incorrect?

Statement-I: Ionization enthalpy of nitrogen is greater than that of oxygen.
Statement-II: Nitrogen has exactly half filled electronic configuration which is more stable than electronic configuration of oxygen.

The hydration enthalpies of alkali metal ions decreases in ______ order.

Quick lime is ________

Select the molecule which has only one \(\pi\) bond.

The general formula for alkadiene is ____________

The IUPAC name of the Compound is _____________
 

The IUPAC name of the compound CH₃ – CH = CH – C ≡ CH is _________

The IUPAC name of the compound \({ H }_{ 3 }C-\overset { \underset { | }{ { CH }_{ 3 } } }{ \underset { \overset { | }{ { CH }_{ 3 } } }{ C } } -CH=C{ \left( { CH }_{ 3 } \right) }_{ 2 }\) is _____________

Balance the following equations by oxidation number method - \({ K }Mno_{ 4 }+{ Na }_{ 2 }{ So }_{ 3 }\longrightarrow { MnO }_{ 2 }+{ Na }_{ 2 }{ So }_{ 4 }+KOH\)

How many electrons in sulphur (z = 16) can have n + 1 = 3?

Oxygen an fluorine have lower electron affinity, then sulphur and chlorine in their respective groups. Explain why?

How is deuterium prepared from heavy water?

Account for the low solubility of lithium fluoride in water.

Which of the group has highest +I effect ?

-I effect is shown by ____________.

Assertion : Tertiary Carbocations are generally formed more easily than primary Carbocations ions.
Reason : Hyper conjugation, as well as inductive effect due to additional alkyl group, stabilize tertiary carbonium ions.
(a) both assertion and reason are true and reason is the correct explanation of assertion.
(b) both assertion and reason are true but reason is not the correct explanation of assertion.
(c) Assertion is true but reason is false
(d) Both assertion and reason are false

Which of the following represent a set of nuclephiles ?

The geometrical shape of carbocation is ______________.

What is the hybridisation state of benzyl carbonium ion ?

Decreasing order of nucleophilicity is ____________.

Homolytic fission of covalent bond leads to the formation of ___________.

Hyper Conjugation is also known as ___________.

Which of the following species does not exert a resonance effect ?

Define gram equivalent mass of an element.

How does ionisation energy vary in a group?

Ice is less dense than water at O°C. Justify this statement.

The hydroxides and carbonates of sodium and potassium are easily soluble in water while the corresponding salts of magnesium and calcium are sparingly soluble in water. Explain

Most aeroplanes cabins are artificially pressurized. Why?

Cis – 2 – butene and trans – 2 – butene are __________

\(\underset { \overset { | }{ Br } }{ { CH }_{ 2 } } -\underset { \overset { | }{ Br } }{ { CH }_{ 2 } } \overset { \left( A \right) }{ \longrightarrow } CH\equiv CH,\) where A is ___________

In which of the following molecules, all atoms are co-planar ___________

Which of the following compounds will not undergo Friedal – crafts reaction easily?(NEET)

Categorise the redox reactions that occur in our daily life

Calculate the total number of angular nodes and radial nodes present in 3p-orbital.

The number of elements in the first period is only 2. Give reason.

What is hydrogen bonding?

8 g of methane is placed in a 5 litre container at 27° C. Find Boyle's constant.

\({ C }_{ 2 }{ H }_{ 5 }Br+2Na\overset { dry\quad ether }{ \longrightarrow } { C }_{ 4 }{ H }_{ 10 }+2NaBr\) The above reaction is an example of which of the following

The C – H bond and C – C bond in ethane are formed by which of the following types of overlap _________

Which of the following is optically active _________

The general formula for cyclo alkanes _________

Which of the following compounds shall not produce propene by reaction with HBr followed by elemination (or) only direct elimination reaction (NEET)__________

Calculate the equivalent weight of H₃PO₄ and Ca(OH)₂ on the basis of given reaction.
H₃PO₄ + NaOH \(\longrightarrow\) NaH₂PO₄ + H₂O
Ca(OH)₂ + HCI \(\longrightarrow\) Ca(OH)CI + H₂O

In Rutherford's experiment, generally thin foil of heavy atoms, like gold, platinum etc. have been used to bombard the a-particles. If the thin foil of light atoms like aluminum is used, what difference would be observed from the above results?

What are all the factors that influences electron gain enthalpy?

What causes the temporary and permanent hardness of water?

Explain the Castner-Kellner process of manufacturing sodium hydroxide.

In the reaction  X is ________.

The treatment of ethyl formate with excess of RMgX gives ____________

The name of C₂F₄Cl₂ is ___________

Match the compounds given in Column I with suitable items given in Column II

Consider the reaction,
CH₃CH₂CH₂Br + NaCN → CH₃CH₂CH₂CN + NaBr
This reaction will be the fastest in __________

The oxidation state of a element in its uncombined state is

Fe2 + \(\longrightarrow\) Fe³⁺ + e^- is a ________ reaction.

Assertion : Fluorine has an oxidation state of - 1 in all its compounds.
Reason : Fluorine is the most electronegative element of the periodic table.

The oxidation number of oxygen in O₂ is__________

The oxidation number of hydrogen in LiH is _________

Write note on decomposition reaction

Write a note on limitations of Bohr's atom model.

Given the bona lengths of H₂, Cl₂, C - C bond in diamond, Si - C bond in carborundum and C - CI bond in CCl₄ are 0.74, 1.9, 1.54, 1.93 and 1.76A respectively, find the covalent radius of hydrogen, chlorine, carbon in diamond, silicon and carbon in CCI₄.

Compare the structures of ice & water

Explain the preparation and uses of the following compounds of calcium.

The carbo cation formed in SN¹ reaction of alkyl halide in the slow step is ________

The major products obtained when chlorobenzene is nitrated with HNO₃ and con H₂SO₄.

Which one of the following is most reactive towards nucleophilic substitution reaction?

The raw material for Rasching process _________

acetone \(\overset { i){ CH }_{ 3 }Mgl }{ \underset { ii){ H }_{ 2 }O/{ H }^{ -1 } }{ \longrightarrow } } X,\) X is _________

The solid state of matter is converted into gas by

Identify the incorrect statement about a compound.

The characteristic feature of orderly arrangement of molecules belongs to ______________.

Which form of based on physical characteristics possess neither definite volume nor definite shape?

12 g of carbon-12 contains_____carbon atoms

Balance the following equations by oxidation number method.
KMnO₄ + KOH + H₂O₂ ⟶ K₂MnO₄ + O₂ + H₂O

Explain the angular distribution function of 1s, 2s, 3s, 2p, 3d and 4f orbits.

Distinguish between electron affinity and electron negativity.

Give the chemical properties of heavy water and water.

Describe Solvay process (or) how is washing soda (or) sodium carbonate prepared in industries?

Which sequence for green house gases is based on GWP ?

The pH of normal rain water is ________

Identify the wrong statement in the following __________.

Release of oxides of nitrogen and hydrocarbons into the atmosphere by motor vehicles is prevented by using __________.

Match the List I with List II and select the correct answer using the code given below the lists.

Haemoglobin of the blood forms carboxy haemoglobin with __________.

Photo chemical smog formed in congested metropolitan cities mainly consists of ___________

Ozone depletion will cause ___________.

Living in the atmosphere of CO is dangerous because it __________.

Biochemical oxygen Demand value less than 5 ppm indicates a water sample to be ___________.

How many nodes are possible for 2s orbital?

The subsidiary quantum number decides ______

As per Aufbau principle, arrange the orbitals in increasing order of energy __________

In multi-electron atom,4s-orbital is lower in energy than __________

Shape of an orbital is given by ____________

What do you understand by the term mole ?

What do you understand by the term oxidation number ?

Distinguish between oxidation and reduction.

The density of carbon dioxide is equal to 1.965 kgm^-3 at 273 K and 1 atm pressure. calculate the molar mass of CO₂.

Calculate the average atomic mass of naturally occurring magnesium using the following data.

Define relative atomic mass.

Define equivalent mass.

Distinguish between oxidation and reduction.

Which contains the greatest number of moles of oxygen atoms
i) 1 mol of ethanol
ii) 1 mol of formic acid
iii) 1 mol of H₂O

Hydrogen peroxide is an oxidising agent. It oxidises ferrous ion to ferric ion and reduced itself to water. Write a balanced equation.

The de-Broglie wavelength of a particle with mass 19 and velocity 100 m/s is __________

Which of the following is not among short comings of Bohr's model?

What will be the wavelength of a ball of mass 0.1 kg moving with a velocity of 10ms^-1?

The de-Broglie wavelength associated with a matter particle is ______________

The wavelength associated with an electron moving with velocity 10¹⁰ ms^-1 is ___________

Define orbital ? what are the n and 1 values for 3p_x and 4d_x²-y² electron ?

How many orbitals are possible for n = 4?

Which quantum number reveal information about the shape, energy, orientation and size of orbitals?

For each of the following, give the sub level designation, the allowable m values and the number of orbitals
(i) n = 4, l = 2
(ii) n = 5, l = 3
(iii) n = 7, l = 0

Consider the following electronic arrangements for the d⁵ configuration.
(a)

(b)

(c)

which of these represents the ground state

An element M combines with CI. What would be the formula of the compound obtained if M has a valence of 2?

Law of triad was unable to explain for the element

Law of octaves was proposed by _____

______ proposed modern periodic law.

The atomic weight of Au is ______

The stabilisation of a half filled d - orbital is more pronounced than that of the p-orbital why?

How many radial nodes for 2s, 4p, 5d and 4f orbitals exhibit? How many angular nodes

How fast must a 54g tennis ball travel in order to have a de Broglie wavelength that is equal to that of a photon of green light 5400\(\overset { 0 }{ A } \) ?

Give the electronic configuration of Mn²⁺ and Cr³⁺

An atom of an element contains 35 electrons and 45 neutrons. Deduce
(i) the number of protons
(ii) the electronic configuration for the element
(iii) All the four quantum numbers for the last electron

What is effective nuclear charge?

Is the definition given below for ionisation enthalpy correct?
"Ionisation enthalpy is defined as the energy required to remove the most loosely bound electron from the valence shell of an atom.

Magnesium loses electrons successively to form Mg⁺, Mg²⁺ and Mg³⁺ ions. Which step will have the highest ionisation energy and why?

Define electro negativity.

Give the general electronic configuration of lanthanides and actinides.

Explain why hydrogen is not placed with the halogen in the periodic table.

An the cube at 0° C is placed in some liquid water at 0⁰C, the ice cube sinks - Why? What will happen to ice at 0⁰C placed in liquid water at 0⁰C? 

Predict which of the following hydrides is a gas on a solid
(a) BCI
(b) NaH 
Give your reason.

NH₃ has exceptionally high melting point and boiling point as compared to those of the hydrides of the remaining element of group 15. Explain.

Why interstitial hydrides have a lower density than the parent metal.

Pd has exceptional electronic configuration of 4d¹⁰ 5s⁰ It belongs to period ______ and group _____

The elements at the extreme left of periodic table has strong behaviour ______

On moving diagonally across the periodic table, the second and third period elements show certain similarities. Pick out the pair which shows such a property.

d-block elements form ____ compounds.

X, Y and Z are three members of a Doboreiner's triad. If the atomic mass of X is 7 and that of Z is 39, what in the atomic mass of Y?

Explain what is meant by efflorescence.

Substantiate lithium fluoride has the lowest solubility among group one metal fluorides.

Beryllium halides are Covalent whereas magnesium halides are ionic why ?

An alkali metal (x) forms a hydrated sulphate, X₂SO₄ • 10 H₂O. Is the metal more likely to be sodium (or) potassium.

Why alkaline earth metals are harder than alkali metals.

Name two items that can serve as a model for Gay Lusaac's law and explain.

Give the mathematical expression that relates gas volume and moles.

Can a Van der Waals gas with a = 0 be liquefied? explain

Aerosol cans carry clear warning of heating of the can. Why?

Why do astronauts have to wear protective suits when they are on the surface of moon?

Predict the feasibility of a reaction when
(i) both ΔH and ΔS positive
(ii) both ΔH and ΔS negative
(iii) ΔH decreases but ΔS increases

Define enthalpy of combustion.

Define the calorific value of food. What is the unit of calorific value?

What is lattice energy?

State the third law of thermodynamics.

The half life period of Tritium is ___________

Ammonia is manufactured by __________ process.

___________ torches is/are used in cutting and welding of a steel.

Hydrogen is used in _________

The conversion of atomic hydrogen to dihydrogen is a __________ change.

Define Gibb's free energy.

Define molar heat capacity. Give its unit

Define enthalpy of neutralization

Give Kelvin statement of second law of thermodynamics.

Identify the state and path function out of the following:
a) Enthalpy
b) Entropy
c) Heat
d) Temperature
e) Work
f) Free energy.

Hydrogen accepts an electron to attain the inert gas configuration. In this way it resembles __________

Hydrogen acts as a reducing agent and thus resembles ______________

Which among of the following reaction produces hydrogen?

In which of the following compounds does hydrogen has an oxidation state of -1?

Which properties of hydrogen are responsible for moderation of the climate and body temperature of living beings?

The elements that belong to group 1 of the periodic table are called as _________

Rubidium belongs to______group of metals

The radio active element of group 1 is ______

Half life of francium is _______

Electronic configuration of 1s block of elements is ______

______ ions are found in large proportions in biological fluids,

________ is responsible for the transmission of nerve signals.

Spodumene is the silicate mineral of _____

Which of the following metals is most commonly used in photochemical cells?

Which among the following is the strongest reducing agent?

Compression factor Z is given by _____________

What is the dominant intermolecular force or bond that must be overcome in converting liquid methanol to a gas?

Compressibility factor for CO₂ at 400 K and 71.0 bar is 0.8697 the molar volume of CO₂ under these conditions _____________

When the gas behaves ideally, the compression factor Z is ___________

_____________ is the gas constant.

The compressibility factor for an ideal gas is ______________.

Which of the following pair will diffuse at the same rate?

The value of Vander Waals constant "a" is maximum for __________.

A person living in Shimla observed that cooking food with using pressure cooker takes more time. The reason for this observation is that at high altitude _____________.

Statement-I: At constant temperature, PV vs V plot for real gases is not a straight line.
Statement-II: At high pressure, all gases have Z >1, but at intermediate pressure, most gases have Z < 1.

All naturally occurring processes are _________ process

The process in which no heat can flow into or out of the system are called ___________ process.

The process in which temperature of the system remains constant is called __________ process

For an isothermal process _____

The process in which volume of the system remains constant is called ___________ process

The process in which no heat can flow into or out of the system are called ___________ process.

The process in which temperature of the system remains constant is called __________ process

For an isothermal process _____

The process in which volume of the system remains constant is called ___________ process

Which among the following is not a state function?

In the system; \(Fe\left( OH \right) _{ 3\left( s \right) }\rightleftharpoons { Fe }_{ \left( aq \right) }^{ 3+ }+{ 3OH }_{ \left( aq \right) }\) decreasing the conc. of OH^-ions \(\cfrac { 1 }{ 3 } ^{ - }\)times will cause the equilibrium cone, of Fe³⁺ to increase_____________ times

For the reaction \(CO_{ \left( g \right) }+2H_{ 2\left( g \right) }\rightleftharpoons { CH }_{ 3 }{ OH }_{ \left( g \right) }\) If active mass of CO is kept constant and active mass of H₂ is tripled, the rate of forward reaction will become ____________

For the homogeneous gas reaction at 600K \(4NH_{ 3\left( g \right) }+5{ O }_{ 2\left( g \right) }\rightleftharpoons 4NO_{ \left( g \right) }+6{ H }_{ 2 }{ O }_{ \left( g \right) }\) The unit of equilibrium constant K" is

The equilibrium \({ A }_{ \left( g \right) }+4B_{ \left( g \right) }\rightleftharpoons AB_{ 4\left( g \right) }\) attained by mixing equal moles of A and B in a one litre vessel. Then at equilibrium _____________

If Ar is added to the equilibrium
\({ N }_{ 2g }+{ 3H }_{ 2\left( g \right) }\rightleftharpoons { 2NH }_{ 3 }\) at constant volume, then equilibrium will _____________

What would be the value of ∆n_g for the reaction NH₄CI(s) ⇌ NH₂(g) + HCI(g)?

At 500K, equilibrium constant K_c for the following reaction is 5, \(\frac { 1 }{ 2 } { H }_{ 2 }(g)+\frac { 1 }{ 2 } { I }_{ 2 }(g)\leftrightharpoons { H }I(g)\) what would be the equilibrium constant Kc for the reaction 2HI(g) ⇌ H₂(g) + I₂(g)

For the reaction 2NO₂(g) ⇌ 2NO(g) + O₂(g), K_c = 1.8 x 10^-6 at 185°C. At the same temperature the value of K_c for the reaction. NO(g) + \(\frac{1}{2}\) O₂ ⇌ NO₂(g) is__________.

Which of the following reaction will be favoured at low pressure?

Consider the reaction CaCO₃(s) ⇌ CaO(s) + CO₂(g) is a closed container at equilibrium. What would be the effect of addition of CaCO₃ on the equilibrium?

The tanks used by scuba divers are filled with air diluted with 11.7% He ___________

The blocking of capillaires due to sudden release of bubbles of N₂ gas in blood is known as ______

Which of the following gas should have maximum value for k_H?

The increase in the temperature of the aqueous solution placed in a closed vessel will result in its _________

In a binary solution __________

If solute and solvent interactions are more than solute - solute and solvent - solvent interactions then ___________

Which of the following is correct about a solution showing positive deviation?

Which of the following statment is true?

Among the following mixtures, dipole-dipole as the major inferaction, is present in ________

An azeotropic solution of two liquids has a boiling point lower than either of the boiling points of the two liquids when it __________

Which of the following is a polar molecule?

Identify the pair of species that possess same bond order.

In the formation of ethylene molecule, the carbon atom makes use of___________ hybridisation.

Statement I: N₂, CO and CN^- are having same bond order.
Statement II : Isoelectronic species always have same bond order.

Statement I : Bond angle of BF₃ and NF₃ are different
Statement II : Both the molecules are having different shapes.

Which of the following has maximum number of lone pairs associated with Xe?

During the formation of a chemical bond ________.

Using MO theory, predict which of the following species has the shortest bond length?

Identify the incorrect statement regarding the molecule xeO₄.

Which of the following contains maximum number of lone pairs on the central atom?

Which one of the following pairs represents stereoisomerism?

The correct order of increasing bond length of C-H, C-O, C-C, and C = C is _________

Assertion (A): C₂ Dr CI FI can farm 6 different geometrical isomers.
Reason (R):  Each one structure is geometrical isomer of other five structures.
Codes:
(a) Both A and Rare true and Ris correct explanation of A
(b) Both A and R are true but R is not correct explanation of A.
(c) A is true but R is false
(d) Both A and R are false.

Compounds having boiling points widely apart 40k and above can be purified by________.

Purification of two miscible liqulds possessing very close boiling points can be separated using _________

Which of the following is an example of an organic reaction?

Which of the following is an example ofheterocylic aromatic compound?

Which of the following is an example of non-benzenoid aromatic compound?

Which of the following pair is an example of aromatic compounds?

Which of the following is an example of carbocyclic alicyclic compound?

Which one of the following is an example for negative mesomeric effect ?

Which one of the following electrophile used for nitration of benzene ?

Identify the one which does not come under the organic addition reaction.

Primary alcohols undergo which type of reaction to form alkenes ?

CH₃CHO \(\overset { (o) }{ \longrightarrow } \) CH₃COOH. Identify the type of reaction ?

Which of the following is correct order of the stability of carbocations ?

Which one of the following is correct order of the stability of carbanions ?

Which one of the following is not electrophile ?

Which one of the following is not nucleophile ?

Which one of the following is positively charged electrophiles ?

In E1, reaction, the intermediate formed is ___________

How many structural isomers are possible for the molecular formula C₄H₈ which can undergo ozonolysis?

Actylene reacts with ammonical Cu₂CI₂ to give precipitate of ___________

Carbon-carbon bond length in benzene is ____________

The reasonance energy of benzene is ___________

Which one of the following is not a meta director?

Which one of the following is benzene ring deactivator?

Fine the odd one out:

Which among these is not associated with aliphatic compounds?

Which of the following compounds will exhibit cis-trans isomerism?

The best reagent for converting an alcohol into the corresponding chloride is

The order of correct bond energy of C - X bond is

Identify the compound possessing highest boiling point.

\({ CH }_{ 3 }-{ CH }_{ 3 }-Br\overset { KCN }{ \longrightarrow } X\overset { dil.HCl }{ \underset { \triangle }{ \longrightarrow } } Z\) Z is

NBS is a specific reagent for________________.

Chloropicrin is prepared by adding nitric acid to______________,

Which of the following is an example for polyhalo compounds?

Which of the following is a secondary haloalkane?

How many isomers are possible for the formula C₄H₉Cl?

How many isomers are possible for the formula C₅H₁₁Br?

Calculate the molar mass of the following compounds.
Boric Acid [H₃ BO₃]

Calculate the molar mass of the following compounds.
Sulphuric  Acid [H₂ SO₄]

Balance the following equations by ion electron method
\({ C }_{ 2 }{ O }_{ 4 }^{ 2- }+{ Cr }_{ 2 }{ O }_{ 7 }^{ 2- }\longrightarrow { Cr }^{ 3+ }+{ CO }_{ 2 }\) (in acid medium)

Balance the following equations by ion electron method.
\({ Na }_{ 2 }{ S }_{ 2 }{ O }_{ 3 }+{ I }_{ 2 }\longrightarrow { Na }_{ 2 }{ S }_{ 4 }{ O }_{ 6 }+NaI\)

Balance the following equations by ion electron method 
\(Zn+{ NO }_{ 3 }^{ - }\longrightarrow { Zn }^{ 2+ }+No\)

Balance the following equations by oxidation number method - \({ KMn }O_{ 4 }+{ H }_{ 2 }{ C }_{ 2 }{ O }_{ 4 }+{ H }_{ 2 }{ SO }_{ 4 }\longrightarrow { K }_{ 2 }{ SO }_{ 4 }+{ MnSO }_{ 4 }+{ CO }_{ 2 }+{ H }_{ 2 }O\)

Give a brief account of classification of matter.

Distinguish between a homogeneous and heterogeneous mixture.

Mention the characteristics of a compound.

Why atomic masses are called as relative atomic masses?

How many electrons are present in all subshells (fully filled) with n + l = 5?

Why Pauli exclusion principle is called exclusion principle?

At what distance is the radial probability maximum for 1s orbital? What is this distance called?

Bring out the similarities and dissimilarities between a 1s and 2s orbital.

How many radial f spherical nodes will be present in 5f orbital?

Explain how matter has dual character?

Explain about the significance of de Broglie equation.

How many electrons can be accommodated in the main shell I,m and n?

How many electrons that can be accommodated in the subshell s, p, d, f?

Write the general electronic configuration of s,c ,p, d, and f block elements

Name the first and the last elements in the following periods (n) .
(i) n=:4
(ii) n = 5
(iii) n = 6
(iv) n = 7

Mention the characteristics of 's' block elements.

Mention the characteristics of 'p' block elements

Mention the characteristics of 'd' block elements.

Electron gain enthalpy of F is less negative than Cl. Why?

Electron affinity of oxygen is less negative than sulphur. Justify this statement.

Explain about the factors that affect electronegativity.

Explain about periodic variation of electro negativity across a period.

Explain about the period variation of electronegativity along a group.

At room temperature, Hydrogen reacts very slowly. Explain

Explain the consequences of high enthalpy of H-H bond in terms of chemical reactivity of dihydrogen.

How will you classify water based on the spin of the nuclei of the hydrogen atoms?

Life underneath frozen lakes survive even bitter winter. Justify.

Why does water show high boiling point as compared to hydrogen sulphide? Give reasons for your answer.

Draw the structure of
(i) Acetic acid
(ii) Water

Write a note about gas hydrates.

Give the advantages of future fuel - Hydrogen.

What do you understand by the term 'non-stoichiometric hydrides'? Do you expect this type of bydrides to be formed by alkali metals? Justify your answer.

How does the atomic hydrogen or oxy-hydrogen torch function for cutting and welding purposes? Explain.

Alkali metals give a characteristics colour for a bunsen flame. Explain why?

Explain why alkali metals are very reactive.

Lithium iodide is covalent. Explain why?

Mention the uses of lithium.

Mention the uses of sodium.

Give methods of preparation of beryllium chloride.

How is BeH₂ obtained?

How does the basic nature of the oxides of group 2 elements vary down the group?

How does (i) solubility, (ii) thermal stability, (iii) basic character hydroxides of group 2 elements very down the group.

Beryllium halide are covalent. Explain why?

Identify the elements that are in gaseous state under normal atmospheric conditions.

Distinguish between a gas and a vapour.

Define pressure. Give its units.

Define atmospheric pressure. What is its value?

Deep sea divers ascend slowly and breath continuously by time they reach the surface. Give reason.

Define Graham's law of diffusion.

Helium diffuses more than air. Give reason.

Explain about the applications of Graham's law of diffusion.

What is compression factor?

CO₂ gas cannot be liquefied at room temperature. Give reason.

Explain Zeroth law of thermodynamics.

Define molar heat capacity at constant volume and molar heat capacity at constant pressure.

Explain why C_p is always greater than C_v?

Describe the application of heat of combustion.

Give expressions for the entropy change a-phase change.

What is the condition spontaneity in terms of free energy change?

Why standard entropy of an elementary substance is not zero whereas standard enthalpy of formation is taken as zero?

The equilibrium constant for a reaction is one or more if \(\Delta G^{\ominus}\) for it is less than zero. Explain.

Many thermodynamically feasible reactions do not occur under ordinary conditions. Why?

What is the aim of the study of chemical thermodynamics?

Define the state of equilibrium.

What are the different types of equilibrium? Explain with example?

Explain about the equilibrium involving dissolution of solid in liquid with suitable example.

How is a gas-solution equilibrium exist?

What is meant by active mass? Give its unit.

Show that K_P = K_C with two examples

Give two examples of equilibrium reactions where Kp > K_C

When will be K_P < K_C? Give two example

Write the K_c for the reaction CO₂(g) + H₂O(l) \(\leftrightharpoons \) H^+(aq)+ HCO₃^-(aq).

When will be K_p < K_c? Give two example

why acetic acid deviates from ideal behaviour in solutions ?

why a solution of KCL in water deviates from ideal behaviour ?

Write a short note on Van't Hoff equation

Define colligative properties.

What is abnormal molar mass?

What is mass percentage ?

What do you mean by volume percentage ?

What do you mean by "mass by volume percentage''.

What is meant by ppm? Where is it used?

What is meant by stock solution (or) standard solution? What is meant by working standard?

Identify the magnetic nature of the anion of Na₂O₂.

How is the sequence of energy levels of molecular orbitals written in case of heavier diatomic molecules ?

Bond order increases with loss of electron in bonding molecular orbital - State True or False and give reason.

How does the effect of the process C₂ \(\rightarrow\) C₂⁺ + e^- affect the bond order ?

What are chemical bonds ?

Metals are very good electrical conductors. Why?

Metals have high thermal conductivity. Give reason.

Most metals are black except Cu, Ag and Au. Why ?

Write the favourable factors for the formation of ionic bond.

Although geometries of NH₃ and H₂0 molecules are distorted tetrahedral, bond angle in water is less than that of ammonia. Discuss

What are the methods used for representing the structure of an organic compound?

Define stereoisomerism.

How will you carry out the conversion of cis- isomer into a trans-isomer?

Does propene exhibit geometrical isomers? Give reason.

Generally the trans isomer is more stable than cis isomer. Why?

Explain ring chain isomerism with the formula C₄H₈

Define stereo-isomerism.

Define geometrical isomerism with an example.

Trans isomer is more stable than cis isomer. Justify this statement.

Draw the cis, trans isomeric structures of 1, 3-butadiene.

What are organic reactions?

What is mechanism of the reaction ?

Mention the types of fission of a covalent bond?

Explain the homolytic fission of a covalent bond ?

What are free radical initiators?

Identify the electrophilic centre in the following compound & CH₃ - CH = O, CH₃CN, CH₃I.

Which of the two is expected to be more stable and why ? \({ O }_{ 2 }NC{ H }_{ 2 }C{ H }_{ 2 }\overset { - }{ O } \) (or) \(C{ H }_{ 3 }C{ H }_{ 2 }\overset { - }{ O } \)

Which of the two structures A and B given below is more stabilised by resonance ? Explain.
CH₃COOH (A) and \(C{ H }_{ 3 }CO\overset { - }{ O } \) (B)

Draw the resonating structure of C₆H₅NH₂ .

How will you determine the rate of chemical I reaction ?

Define benzenoid and non-benzenoid compounds with example.

What are activating and deactivating groups?

Show the classification of hydrocarbons.

What are conformation? Explain.

How are branched alkanes formed from normal alkanes?

What is Sabatier- Sendersens reaction?

What are decarboxylation reactions? Given an example.

Write a note on Kolbe's electrolytic method?

How will you prepare propane from Chloropropane?

What is Wurtz reaction?

Write a short note on \(\beta\)-elimination reaction.

How does the haloalkanes react with metals?

How does benzene diazonium chloride react with HBF₄?

Write a note on carbylamine reaction.

Write the IUPAC names of the following compounds.
(i) (CCI₃)₃ CCl
(ii) (CH₃)₃ CCH = C(CI) C₆H₄I- p

Explain Carbylamine reaction.(or) Give the characteristic test for primary amine.

How will you prepare carbon tetrachloride?

How will you convert carbon tetrachloride to chloroform?

What are freons? How are they named? Give two examples

What are ambident nucleophiles? Explain with an example.

Why photochemical smog is called so ?

Write a note on the formation of ozone layer

What is green house effect ?

Write a short note on global warming.

Define stone leprosy and gives its equation.

What are fumes? Give one example.

What are the techniques to reduce particulate pollutants?

How will you control photochemical smog?

What is meant by water pollution?

What is BOD?

State Le-Chatelier principle.

State law of mass action.

Derive a general expression for the equilibrium constant K_P and K_C for the reaction 
3H₂(g) + N₂(g) ⇌ 2NH₃(g).

What is the effect of added inert gas on the reaction at equilibrium at constant volume.

Deduce the Vant Hoff equation.

If there is no change in concentration, why is the equilibrium state considered dynamic?

What is the relation between K_P and K_C. Give one example for which K_P is equal to K_C.

When the numerical value of the reaction quotient (Q) is greater than the equilibrium constant (K), in which direction does the reaction proceed to reach equilibrium?

Consider the following reactions,
H₂(g) + I₂(g) ⇌ 2 HI(g)
In each of the above reaction find out whether you have to increase (or) decrease the volume to increase the yield of the product.

Explain how will you predict the direction of a equilibrium reaction.

The antiseptic solution of iodopovidone for the use of external application contains 10 % w/v of iodopovidone. Calculate the amount of iodopovidone present in a typical dose of 1.5 mL.

At 400 K 1.5 g of an unknown substance is dissolved in solvent and the solution is made to 1.5 L. Its osmotic pressure is found to be 0.3 bar. Calculate the molar mass of the unknown substance.

What is a vapour pressure of liquid ?
What is relative lowering of vapour pressure ?

State Raoult law and obtain expression for lowering of vapour pressure when nonvolatile solute is dissolved in solvent.

What is molal depression constant ? Does it depend on nature of the solute ?

Define the term ‘isotonic solution’.

Explain the effect of pressure on the solubility.

Calculate the molality of a solution containing 7.5 g of glycine (NH₂ - CH₂ - COOH) dissolved in 500 g of water.

How many moles of solute particles are present in one litre of 10^-4 M potassium sulphate ?

Define bond energy.

What is Polar Covalent bond ? explain with example.

Explain resonance with reference to carbonate ion ?

What type of hybridisations are possible in the following geometeries ?
a) octahedral
b) tetrahedral
c) square planer

CO₂ and H₂O both are triatomic molecule but their dipole moment values are different. Why ?

In CH₄, NH₃ and H₂O, the central atom undergoes sp³ hybridisation - yet their bond angles are different. why ?

Draw the M.O diagram for oxygen molecule calculate its bond order and show that O₂ is paramagnetic.

What do you understand by Linear combination of atomic orbitals in MO theory.

What is dipole moment ?

Draw the Lewis structures for the following species.
i) NO₃^–
ii) SO₄^2–
iii) HNO₃
iv) O₃

Explain paper chromatography.

Describe optical isomerism with suitable example.

0.30 g of a substance gives 0.88 g of carbon dioxide and 0.54 g of water calculate the percentage of carbon and hydrogen in it.

0.32 g of an organic compound, after heating with fuming nitric acid and barium nitrate crystals is a sealed tube game 0.466 g of barium sulphate. Determine the percentage of sulphur in the compound.

In the estimation of nitrogen present in an organic compound by Dumas method 0.35 g yielded 20.7 mL of nitrogen at 150 C and 760 mm pressure. Calculate the percentage of nitrogen in the compound.

Write a note on homologous series.

Give the general formula for the following classes of organic compounds
Aliphatic monohydric alcohol

Write the molecular and possible structural formula of the first four members of homologous series of carboxylic acids.

Give the principle involved in the estimation of halogen in an organic compound by carius method.

Explain paper chromatography.

Write short notes on Resonance.

What are electrophiles and nucleophiles ? Give suitable examples for each.

Show the heterolysis of covalent bond by using curved arrow notation and complete the following equations.
Identify the nucleophile is each case.
CH₃ - Br + KOH →

Explain inductive effect with suitable example.

Explain electromeric effect.

How is propyne prepared from an alkyene dihalide?

Describe the mechanism of Nitration of benzene.

Suggest the route for the preparation of the following from benzene.
3 – chloro nitrobenzene

What happens when isobutylene is treated with acidified potassium permanganate?

Describe the conformers of n - butane.

Describe the conformers of n - butane.

Explain Markow nikoff's rule with suitable example.

Write the structures of folowing alkanes.
1) 2, 3 – Dimethyl – 6 – (2 – methyl propyl) decane
2) 5 – (2 – Ethyl butyl) – 3, 3 – dimethyldecane
3) 5 – (1, 2 – Dimethyl propyl) – 2 – methylnonane.

Identify A and B.

How will you distinguish 1 – butyne and 2 – butyne?

Why chlorination of methane is not possible in dark?

Which alkyl halide from the following pair is
i) chiral
ii) undergoes faster S_N2 reaction?

Give reasons for polarity of C-X bond in halo alkane.

What happens when acetyl chloride is treated with excess of CH₃MgI?

What happens when chloroform reacts with oxygen in the presence of sunlight?

In an experiment ethyliodide in ether is allowed to stand over magnesium pieces. Magnesium dissolves and product is formed
a) Name the product and write the equation for the reaction.
b) Why all the reagents used in the reaction should be dry? Explain
c) How is acetone prepared from the product obtained in the experiment.

What are Freons? Discuss their uses and environmental effects

Explain the mechanism of S_N1 reaction by highlighting the stereochemistry behind it

Starting from CH₃MgI, How will you prepare the following?
i) Acetic acid
ii) Acetone
iii) Ethyl acetate
iv) Iso propyl alcohol
v) Methyl cyanide.

Explain the preparation of the following compounds
i) DDT
ii) Chloroform
iii) Biphenyl
iv) Chloropicrin
v) Freon-12

What would happen, if the greenhouse gases were totally missing in the earth’s atmosphere ?

Which is considered to be earth’s protective umbrella ? Why ?

A person was using water supplied by corporation. Due to shortage of water he started using underground water. He felt laxative effect. What could be the cause ?

What is green chemistry ?

Explain how does greenhouse effect cause global warming.

Mass of one atom of an element is 6.645 x 10^-23g. How many moles of element are there in 0.320 kg.

What is the empirical formula of the following?
i) Fructose (C₆ H₁₂ O₆) Found in honey
ii) Caffeine  (C₈ H₁₀ N₄ O₂) a substance found in tea and Coffee 

Calculate the empirical and molecular formula of a compound containing 76.6% carbon, 6.38 % hydrogen and rest oxygen its vapour density is 47.

How many moles of hydrogen is required to produce 10 moles of ammonia ?

How much volume of chlorine is required to form 11.2 L of HCI at 273 K and 1 atm pressure?

In a reaction x + y + z₂ \(\longrightarrow \) xyz₂ identify the Limiting reagent if any, in the following reaction mixtures.
i) 200 atoms of x + 200 atoms of y + 50 molecules of z₂
ii) 1 mol of x + 1 mol of y + 3 mol of z₂
iii) 50 atoms of x + 25 atoms of y + 50 molecules of z₂
iv)  2.5 mol of x + 5 mol of y + 5 mol of z₂

What is the difference between molecular mass and molar mass ? Calculate the molecular mass and molar mass for carbon monoxide.

How many moles of ethane is required to produce 44 g of CO_2(g) after combustion.

Calculate the amount of water produced by the combustion of 32 g of methane.

How much volume of carbon dioxide is produced when 50 g of calcium carbonate is heated completely under standard conditions ?

State and explain pauli exclusion principle.

Explain briefly the time independent schrodinger wave equation?

Show that the circumference of the Bohr orbit for the hydrogen atom is an integral multiple of the de Broglie wave length associated with the electron revolving arround the nucleus.

The quantum mechanical treatment of the hydrogen atom gives the energy value:
\({ E }_{ n }=\frac { -13.6 }{ { n }_{ 2 } } ev{ \ atom }^{ -1 }\)
(i) use this expression to find ΔE between n = 3 and n = 4
(ii) Calculate the wavelength corresponding to the above transition.

Determine the values of all the four quantum numbers of the 8^th electron in O- atom and 15^th electron in Cl atom.

The electronic configuration of atom is one of the important factor which affects the value of ionisation potential and electron gain enthalpy. Explain.

In what period and group will an element with Z = 118 will be present?

Elements a, b, c and d have the following electronic configurations:
a: 1s², 2s², 2p⁶
b: 1s², 2s², 2p⁶, 3s², 3p¹
c: 1s², 2s², 2p⁶, 3s², 3p⁶
d: 1s², 2s², 2p¹
Which elements among these will belong to the same group of periodic table.

Why halogens act as oxidising agents?

Mention any two anomalous properties of second period elements.

What is water-gas shift reaction?

Give the uses of heavy water?

How do you convert para hydrogen into ortho hydrogen?

How do you expect the metallic hydrides to be useful for hydrogen storage?

Do you think that heavy water can be used for drinking purposes?

Write the expected formulas for the hydrides of 4^th period elements. What is the trend in the formulas? In what way the first two members of the series different from the others?

Hydrogen peroxide can function as an oxidising agent as well as reducing agent. substantiate this statement with suitable examples.

What are isotopes? Write the names of isotopes of hydrogen.

Explain the exchange reactions of deuterium.

Mention the uses of deuterium.

Give the systematic names for the following
Milk of magnesia

Mention the uses of plaster of paris

Why sodium hydroxide is much more water soluble than chloride ?

Write the chemical equations for the reactions involved in solvay process of preparation of sodium carbonate.

Which would you expect to have a higher melting point magnesium oxide or magnesium fluoride ? Explain your reasoning.

Would it be easier to drink water with a straw on the top of Mount Everest?

A sample of gas has a volume of 8.5 dm³ at an unknown temperature. When the sample is submerged in ice water at 0 °C, its volume gets reduced to 6.37 dm³. What is its initial temperature ?

Sulphur hexafluoride is a colourless, odourless gas; calculate the pressure exerted by 1.82 moles of the gas in a steel vessel of volume 5.43 dm³ at 69.5°C, assuming ideal gas behaviour.

Hydrochloric acid is treated with a metal to produce hydrogen gas. Suppose a student carries out this reaction and collects a volume of 154.4 x 10^-3 dm³ of a gas at a pressure of 742 mm of Hg at a temperature of 298 K. What mass of hydrogen gas (in mg) did the student collect ?

A combustible gas is stored in a metal tank at a pressure of 2.98 atm at 25°C. The tank can withstand a maximum pressure of 12 atm after which it will explode. The building in which the tank has been stored catches fire. Now predict whether the tank will blow up first or start melting? (Melting point of the metal = 1100 K).

Balance the following equations by oxidation number method.
KMnO₄ + KOH + H₂O₂ ⟶ K₂MnO₄ + O₂ + H₂O

Explain the angular distribution function of 1s, 2s, 3s, 2p, 3d and 4f orbits.

Distinguish between electron affinity and electron negativity.

Give the chemical properties of heavy water and water.

Describe Solvay process (or) how is washing soda (or) sodium carbonate prepared in industries?

Write note on decomposition reaction

Write a note on limitations of Bohr's atom model.

Given the bona lengths of H₂, Cl₂, C - C bond in diamond, Si - C bond in carborundum and C - CI bond in CCl₄ are 0.74, 1.9, 1.54, 1.93 and 1.76A respectively, find the covalent radius of hydrogen, chlorine, carbon in diamond, silicon and carbon in CCI₄.

Compare the structures of ice & water

Explain the preparation and uses of the following compounds of calcium.

Calculate the equivalent weight of H₃PO₄ and Ca(OH)₂ on the basis of given reaction.
H₃PO₄ + NaOH \(\longrightarrow\) NaH₂PO₄ + H₂O
Ca(OH)₂ + HCI \(\longrightarrow\) Ca(OH)CI + H₂O

In Rutherford's experiment, generally thin foil of heavy atoms, like gold, platinum etc. have been used to bombard the a-particles. If the thin foil of light atoms like aluminum is used, what difference would be observed from the above results?

What are all the factors that influences electron gain enthalpy?

What causes the temporary and permanent hardness of water?

Explain the Castner-Kellner process of manufacturing sodium hydroxide.

Categorise the redox reactions that occur in our daily life

Calculate the total number of angular nodes and radial nodes present in 3p-orbital.

The number of elements in the first period is only 2. Give reason.

What is hydrogen bonding?

8 g of methane is placed in a 5 litre container at 27° C. Find Boyle's constant.

Define gram equivalent mass of an element.

How does ionisation energy vary in a group?

Ice is less dense than water at O°C. Justify this statement.

The hydroxides and carbonates of sodium and potassium are easily soluble in water while the corresponding salts of magnesium and calcium are sparingly soluble in water. Explain

Most aeroplanes cabins are artificially pressurized. Why?

Balance the following equations by oxidation number method - \({ K }Mno_{ 4 }+{ Na }_{ 2 }{ So }_{ 3 }\longrightarrow { MnO }_{ 2 }+{ Na }_{ 2 }{ So }_{ 4 }+KOH\)

How many electrons in sulphur (z = 16) can have n + 1 = 3?

Oxygen an fluorine have lower electron affinity, then sulphur and chlorine in their respective groups. Explain why?

How is deuterium prepared from heavy water?

Account for the low solubility of lithium fluoride in water.

One 'U' stands for the mass of ______________.

Which of the following about the electron is incorrect?

Statement-I: Ionization enthalpy of nitrogen is greater than that of oxygen.
Statement-II: Nitrogen has exactly half filled electronic configuration which is more stable than electronic configuration of oxygen.

The hydration enthalpies of alkali metal ions decreases in ______ order.

Quick lime is ________

Assertion : Fluorine has an oxidation state of - 1 in all its compounds.
Reason : Fluorine is the most electronegative element of the periodic table.

In Rutherford's gold foil experiment, a thin gold foil was bombarded with a stream of fast moving ___________

The statement that is not correct for modern classification of element is
(1) The properties of elements are periodic function of these atomic numbers.
(2) The ionisation enthalpy of the elements generally increase with increase in atomic number
(3) For transition elements the 3d orbitals are filled after 3p-orbitals and befire 4s orbitals.
(4) Fifth period contain 18 elements.

___________ torches is/are used in cutting and welding of a steel.

Half life of francium is _______

Explain about Kossel-Lewis approach to chemical bonding.

Explain about the salient features of molecular orbital theory.

Draw the M.OI. diagram of No molecule. Calculate its bond order and show that its paramagnetic.

Explain about metallic bonding

Explain about the bonding in metals by molecular orbital theory.

Explain about valence bond theory for the formation of H₂ molecule.

What are the salient features of Valence Bond (VB) theory?

Explain about sp hybridisation with suitable example.

Draw the lewis structure for
Sulphur trioxide (SO₃)

Draw the lewis structure for
Phosphoric acid

Explain about the factors that are responsible for deviation from Raoult's law.

How will you obtain the molecular mass of a solute from relative lowering of vapour pressure ?

Derive an expression for molecular weight of the solute from osmotic Pressure.

What are ideal and non-ideal solutions ? Explain with suitable diagram the behaviour of ideal solutions.

Explain with a suitable diagram and appropriate example, why some non-ideal solution shows positive deviation from Raoult's

How does the change in temperature affect the solubility of a solute in a liquid solvent and gaseous solute in liquid solvent? Explain.

"Rate of vapourisation is reduced by presence of non-volatile solute"- Explain,

Explain the nature of non - ideal solution with positive deviation from Raoult,s law.

(i) When does a non-ideal solution is said to show a negative deviation?
(ii) Analyse the deviation observed in the solution of phenol and aniline.

Explain the various factors which are responsible for the deviation of solution from Raoult's law.

Derive the K_p and K_c for the following equilibrium reaction.
\({ H }_{ 2\left( g \right) }+{ I }_{ 2\left( g \right) }\rightleftharpoons { 2HI }_{ \left( g \right) }\)

Derive the expressions for K_c and K_p for the dissociation of PCI₅

(i) Describe the effect of
(a) addition of H₂,
(b) addition of CH₃0H
(c) removal of CO
(d) removal ofCH₃OH on the equilibrium of
the reaction, \({ 2H }_{ 2(g) }+{ CO }_{ (g) }\rightleftharpoons { CH }_{ 3 }{ OH }_{ (g) }\)
(ii) What happens to an equilibrium in a reversible reaction if a catalyst is added to it?

At certain temperature and under a pressure of 4 atm, PCl₅ is 10% dissociated. Calculate the pressure at which PCls will be 20% dissociated at temperature remaining constant.

What is the equilibrium concentration of each of the substances in the equilibrium when the initial concentration of ICI was 0.78 M?
2 ICI(g) ⇌ I₂(g) + Cl₂(g); K_C = 0.14

Explain: How does the extent of reaction depend on K_c?

PCI₅ PCl₃ and Cl₂ are at equilibrium at 500 K and having concentration 1.59M PCI₃ , 1.59M Cl₂ and 1.41M PCI_5. Calculate Kc for the reaction PCI₅ ⇌ PCl₃ + Cl_2.

Derive K_c and K_p expressions for the equilibrium: x_A+ y_B ⇌ lC+ mD

Derive the expressions for K_C and K_P, for the synthesis of Hl.

Derive the values of K_p and K_c for dissociation of PCl_5.

Discuss in detail about the variation of internal energy with respect to various thermodynamic processes

Write down the conventions that are followed while framing a thermo chemical equation

Explain the measurement of heat change at constant pressure with a neat diagram.

The enthalpy of combustion for H₂, C_(graphite) and CH₄ are -285.8, -393.5 and -890.4 kJ mol^-1respectively. Calculate the standard enthalpy of formation \(\Delta { H }_{ f }^{ 0 }\) for CH₄

Calculate the lattice energy of MgBr₂ from the given data

If an automobile engine burns petrol at a temperature of 816° C and if the surrounding temperature is 21° C, calculate its maximum possible efficiency

Calculate the entropy change in the engine that receives 957.5 kJ of heat reversibly at 110°C temperature.

Calculate the standard entropy change for the following reaction (Δs_f⁰), given the standard entropies of CO_2(g) ,  C_(s) 'O_2(g) as 213.6, 5.740, and 205 JK^-1 respectively.

Calculate the entropy change during the melting of one mole of ice into water at 0°C and 1 atm pressure. Enthalpy of fusion of ice is 6008 J mol^-1.

The entropy change in the conversion of water to ice at 272 k for the system is -22.88 Jk^-1mol^-1 and that of surrounding is + 24.85 Jk^-1 mol-¹, State whether the process is spontaneous or not?

The van der waal's constant 'b' for oxygen is 0.0318 L mol^-1. Calculate the diameter of the oxygen molecule.

An LPG cylinder containing 15 kg of butane at 27° C and 10 atmpressure is leaking. After one day, its pressure is decreased to 8 atm. How much quality of the gas is leaked ?

Arrive at the values of gas constant (R) in dm³ atm mol^-1 K^-1, Pa, m³ K^-1, mol^-1 at JK^-1 mol^-1.

Explain Andrew's isotherm of carbon dioxide.

Express mathematically Dalton's law of partial pressures.

Explain P-V relationship experiments of Robert Boyle.

Derive the ideal gas equation by combining the empirical gas laws.

Using the ideal gas equation how will you calculate the values of R ?

Defined the following terms.

Explain Andrew's isotherm.

Illustrate the role of sodium and potassium in biological fluid

How is sodium hydroxide prepared commercially from brine solution?

Compare the properties of beryllium with other elements of the same group.

Explain the preparation and uses of the following compounds of calcium.

When water is added to compound (A) of calcium, compound B is formed with a hissing sound and evolution of large amount of heat. When CO₂ is passed into the solution, it turns milky due to the formation of compound C. If excess CO₂ is passed into the solution, milkiness disappears due to the formation of compound (D). Identify the compounds A, B, C and D. Explain why the milkiness disappears in the last step.

List out the uses of alkali metals

How are peroxides and superoxides formed by alkali metals?

The hydrides of alkali metals behave as strong reducing agents - Justify the statement.

When does the blue coloured ammonia solution (of alkali metals) changes to bronze colour?

Bring out the simularities between lithium and magnesium.

Explain about Hydrogen sponge

How are reducing agents in synthetic organic chemistry prepared?

How does water react with
(i) SiCI₄
(ii) P₄O₁₀

Explain about the structure of CuSO₄.5H₂O

How is hydrogen peroxide prepared on industrial scale?

Why hard water is not suitable for laundry ?

Explain the laboratory preparation of hydrogen.

Explain the action of water on
1) Na
2) Ba
3) Fe
4) Pb & Cu
5) Ag, Au,& Hg & Pt
6) C, S, & P

Give the chemical properties of heavy water and water.

Calculate
(i) Concentration of H₂O₂ in g/L 
(ii) Normally

Explain about the anomalies of Mendeleev's periodic table.

Explain about the structural features of Moseley's long form of periodic table.

Explain the merits of Moseley's long form of periodic table.

Explain about the general characteristics of periods.

Explain about the salient features of groups.

Give the structural features of modern periodic law.

Mention Anomalies of Mendeleev's periodic table.

How do you classify of elements into blocks? Give their electronic configuration.

Give the characteristics of p-block elements.

Give any five characteristic properties of inner transition elements.

Calculate the de-Broglie wavelength of an electron that has been accelerated from rest through a potential difference of 1 keV.

Calculate the uncertainty in the position of an electron, if the uncertainty in its velocity is 5.7 x 10⁵ ms^-1.

Calculate the total number of angular nodes and radial nodes present in 3d and 4f orbitals.

Explain about
(i) Magnetic quantum number
(ii) Spin quantum number

Explain the angular distribution function of 1s, 2s, 3s, 2p, 3d and 4f orbits.

Enlist the postulates of Bohr's atom model.

By applying Bohr's postulates, arrive at the radius of n^th orbit for hydrogen like atom

Write a note on limitations of Bohr's atom model.

Derive an equation for the wavelength of a matter wave.

List out the important features of quantum mechanical model of atom

Balance the following equations by oxidation number method.
Zn + HNO₃ ⟶ Zn(NO₃)₂ + N₂O + H₂O

Balance the following equations by oxidation number method.
Ag + HNO₃ ⟶ AgNO₃ + H₂O + NO

Balance the following equations by oxidation number method.
K₂Cr₂O₇ + FeSO₄ + H₂SO₄ ⟶ K₂SO₄ + Cr₂(SO₄)₃ + Fe₂(SO₄)₃ + H₂O

Balance the following equations by oxidation number method.
KBr + MnO₂ + H₂SO4 ⟶ KHSO₄ + MnSO₄ + H₂O + Br₂

Balance the following equations by oxidation number method.
KMnO₄ + KOH + H₂O₂ ⟶ K₂MnO₄ + O₂ + H₂O

Write note on combination reaction.

Write note on decomposition reaction

Explain displacement reaction ? Explain its two types with an example for each.

What are disproportionation reaction (or) auto redox reactions ? Give examples.

Arrange the elements silver, Zinc and copper in the order of their decreasing electron releasing tendency and justify your arrangement with an appropriate experiment.

Explain about lassaigne's test for detection of nitrogen in an organic compound.

Explain about the estimation of carbon and hydrogen.

Explain about the estimation of halogens by carius method.

How will you estimate phosphorous in an organic compound?

Explain Dumas method of estimation of nitrogen.

List down the characteristics possessed by the organic compounds.

Explain the following with example.
(i) Fisher projection formula
(ii) Saw horse projection formula
(iii) Newman projection formula

Describe tautomerism with relevant examples.

How would you estimate the percentage of carbon and hydrogen in an organic compound?

How would you estimate the percentage of sulphur in an organic compound by Carius method?

Explain the types of substitution reaction ?

For the following bond cleavages use curved-arrows to show the electron flow and classify each as homolytic or heterolytic fission. Identify reactive intermediate produced as free radical, carbocation and carbanion ?
(a) \({ CH }_{ 3 }O-O{ CH }_{ 3 }\longrightarrow { CH }_{ 3 }\overset { \bullet }{ O } +{ CH }_{ 3 }\overset { \bullet }{ O } \) 
(b)

(c)

(d)

An organic compound (A) has a molecular formula C₂H₆0 it is one of the primary alcohol. A reacts with acidified potassium dichromate to give B. B on further undergoes to oxidation reaction to give C. C on reacts with SOCl₂ to give D which is chlorinated product. Identify A,B,C and D, explain with equation.

An organic compound (A) of a molecular formula C₂H₄ which is a simple alkene. A reacts with dil H₂SO₄ to give B. A again reacts with Cl₂ to give C. Identify A,B and C and write the equations.

Complete the reactions and identify the products.
(i)

(ii)
\({ CH }_{ 3 }-\underset { \overset { | }{ Cl } }{ C } H-{ CH }_{ 3 }\overset { { H }^{ + }/{ K }_{ 2 }{ Cr }_{ 2 }{ O }_{ 7 } }{ \longrightarrow } A\overset { (O)) }{ \longrightarrow } B\)

Explain electron movement in organic reactions.

How does inductive effect influence the reactivity and acidity of carboxylic acids ?

How is resonance useful in explaining the acidity of phenol ?

How does hyper conjugation effect explain the stability of alkenes ?

Explain the types of addition reactions ?

Explain the acidic nature of alkynes.

Write the mechanism of chlorination of benzene.

Describe the mechanism of sulphonation of benzene.

Describe the mechanism of Freidel craft's alkylation.

Write the mechanism of Freidel craft's acylation

Explain various methods of preparation of alkane.

Discuss in detail about the conformations exhibited by ethane.

How are alkene's obtained by Kolbe's electrolytic method (or) How will you Prepare ethene fro Potassium succinate?

How is the structure of benzene elucidated?

Explain in detail about the addition of hydrogen halide to an unsymmetrical alkene.

The simplest aromatic hydrocarbon C₆H₆ reactsⒷ on treatment with sodium hydroxide will (C₆H₅OH), Phenol, © as the product. Also Cl₂ to giveⒶ which on reaction with sodium hydroxide gives Ⓑ.Ⓑ of molecular formula C₆H₆O. @ on treatment with ammonia will give C₆H₇N as @. Identify Ⓐ, Ⓑ, ©, and explain the reactions involved.

An organic compound Ⓐ of molecular formula C₂H₂ reacts with HCI to give C₂ H₄Cl₂ asⒷ.Ⓑon reaction with aqueous KOH will give C₂H₄Oas Ⓒ Identify Ⓐ,Ⓑ, © and explain the reactions involved.

Two isomers of formula C₄H₉ Br are Ⓐ and B, Ⓐ on reaction with alcoholic KOH gives of molecular formula C₄H₈by E₁ reaction. .Ⓑ on reaction with alcoholic KOH gives Ⓓ and Ⓔ as products by Saytzeff's rule. Identify A, B, C, D, E

A simple aromatic hydrocarbon Ⓐ reacts with Cl₂ to give @ of molecular formula C₆H₅Cl.Ⓑ on reaction with ethyl chloride along with sodium metal gives © of formula C₈H₁₀. © alone reacts with Na metal in the presence of ether to give © C₁₂H₁₀. Identify Ⓐ, Ⓑ, © & Ⓓ

An organic compound Ⓐ of molecular formula CH₂O reacts with methyl magnesium iodide followed by acid hydrolysis to give Ⓑ of molecular formula C₂H₆0. Ⓑ on reaction with PCIs gives ©. ©on reaction with alcoholic KOH gives Ⓓan alkene as the product. Identify Ⓐ, Ⓑ ©, Ⓓ and explain the reactions involved.

Explain the classification of organic compounds with example.

Explain SN₂ mechanism with suitable examples.

SN₂ reaction of an optically active haloalkane is accompanied by inversion of configuration at the asymmetric centre. Prove it.

Explain E₂ reaction mechanism with a suitable example.

Describe E₁ reaction mechanism with a suitable example

List out some methods that you suggest to control water pollution in your locality.

Explain about the different layers of Earth's atmosphere.

What are the health effects of particulate pollutants?

What are the effects of photochemical smog?

Explain about the environmental impacts of ozone depletion.

What is environmental pollution ? How is it caused ?

Discuss in detail about the gaseous air pollutants.

What is acid rain ? How is caused ? Enlist its harmful effects ?

What are non-viable particulates ? How are they classified ? Explain.

Discuss the health hazards caused by particulate pollutants.

Explain how styrene is produced by traditional and greener routes ?

How acetaldehyde is commercially prepared by green chemistry?

What do you mean by ozone hole? What are its consequences?

What is photochemical smog? What are its effects ? How can it be controlled ?

(a) Define eutrophication and pneumoconiosis.
(b) Write differences between photochemical smog and classical smog

Explain how hydrocarbons pollute the atmospheric air.

Write notes about great London smog.

What are the effects of classical smog ?

Explain how oxides of nitrogen are introduced directly into the stratosphere?

How chemical wastes pollute water?

What are the uses of freons?

What is DDT? How is it prepared?

Mention the uses of DDT.

Write the equations for the preparation of l-iodobutane from.

Explain why:
(i) the dipole moment of chlorobenzene is lower than that of cyclohexyl chloride?
(ii) alkyl halides though polar, are immiscible with water?
(iii) Gringard reagents should be prepared under anhydrous conditions?

Explain the hydrolysis of 2-bromobutane with aqueous KOH.

Explain the action of alcoholic KOH with 2-bromobutane.

Mention the uses of chloroform

What are the uses of carbon tetrachloride?

What are ogranometallic compounds? Give one example: Explain the nature of the carbon-metal bond.

Explain the polymerisation of acetylene. write notes on
i) Linear polymerisation ii) Cyclic polymerisation

Discuss the Kekule's structure of benzene.

Why benzene undergoes substitution reaction rather than addition reactions under normal conditions?

Explain the industrial preparation of benzene from coal tar.

Explain the sulphonation of benzene.

Write a brief note on polymerisation of alkenes.

How many types of polymerisation are possible in alkynes?

State Huckel's rule of aromaticity and explain it interms of cyclopentadiene, cycloxtateraene and cyclopropenylcation.

Among anthracene and cyclopentadiene which is aromatic? Give reason for your answer.

Explain the molecular orbirtal structure of benzene.

Carry over the following reaction mechanisms.
(i) Bromination of alkene
(ii) Addition of HCN to CH₃CHO
(iii) Formation of alkyl bromide with benzoyl peroxide as radical initiator.

Which of the following compounds will not exist as resonance hybrid? Give reason for your answer.
(i) CH₃ - OH
(ii) R-CONH₂
(iii) CH₃-CH = CH-CH₂NH₂

Which bond is more polar in the following pair of molecular?
(i) H₃C-H (or) H₃C-Br
(ii) H₃C-NH₂ (or) H₃C-OH
(iii) H₃C-OH (or) H₃C-SH

Write structures of various carbocations that can be obtained from 2-methyl butane. Arrange these carbocations in order of increasing stability.

The structure of triphenylmethyl cation is given below. This very stable and some of its salts can be stored for months. Explain the cause of high stability of this cation.

While writing the resonance structures, what are the rules to be followed ?

Distinguish between electrophiles and nucleophiles

Illustrate with examples, the three types of electron movement in organic reaction.

Discuss the reason behind the classification of inductive effect into +I and -I effect.

Explain the different types of substitution reactions or displacement reactions.

Discuss the conditions for optical isomerism.

How would you detect the presence of carbon and hydrogen in a compound?

(i) Give the test to predict the .presence of Cl, Br and I in an organic compound.
(ii) How will you eliminate in Nand S present in an organic halogen compund?

Explain how benzoic acid (or Naphthalene or camphor) purified. (or) Explain how a substance is purified by sublimation.

Suggest and explain the method suitable to purify the organic compounds depending on their boiling points.

What is the difference between distillation, distillation under reduced pressure and steam distillation?

How will you derive the molecular structure from the type of hybridisation?

Define the term isomerism and write a short note on its classification.

Write a short note on homologous series.

Write a note on cis-trans isomerism in oximes and azo compounds.

Distinguish between a sigma bond and a pi bond.

Write the important conditions required for the linear combination of atomic orbitals to form molecular orbitals.

What are Lewis structures? Write the Lewis structure of H₂, BeF₂ and H₂O.

What are the main postulates of Valence Shell Electron Pair Repulsion (VSEPR) theory ?

Explain why BeH₂ molecule has a zero dipole moment although the Be - H bonds are polar.

Draw the lewis structure of
(i) Ammonia
(ii) Methane
(iil) Dinitrogen pentoxide.

Calculate the bond enthalpy of OH bond in water.

Explain how the ionic character in a covalent bond is related to electronegativity?

CuCI is more covalent than NaCl. Give reason.

Explain the bonding in oxygen molecule.

What are gaseous solution ? Give its various types with example.

What are liquid solutions ? Explain with example.

What are solid solution ? Give example.

How will you prepare a standard solution ?

What are the advantages of standard solution.

Enlist the advantages using standard solutions.

Write a note on solubility of solute and brief out the formation of a saturated solution with an example.

Explain the above variation in solubility with respect to temperature for selective compounds.

With the help of a graph discuss the variation of vapour pressure of benzene in toluene.

Discuss the comparison between Raoult's law and Henry's law.

Explain the effect of concentration of reactants on an equilibrium with example

Consider the reaction, N₂(g) + 3H₂(g) ⇌ 2NH₃(g). Explain the effect of pressure on this equilibrium reaction.

Why pressure has no effect on the synthesis of HI?

Explain the effect of temperature on the following equilibrium reaction.
N₂(g) + 3H₂Cg)⇌ 2NH₃(g)Δ H = - 92.2 kJ.

How does oxygen exchanges between maternal and fetal blood in a pregnant women ?

What happens when the' concentration of H₂ and I₂ are increased in the reaction \({ H }_{ 2 }+{ I }_{ 2 }\rightleftharpoons 2HI?\)

Discuss the changes you observe in the reaction of I synthesis of ammonia with preference to effect of pressure.

Write a note on Haber's process emphasizing the idea of effect of a catalyst in an equilibrium reaction.

What inferences do you observe by the values of Q andK_c?

Explain about th formation of solid-liquid equilibrium with suitable example.

Define entropy of fusion.

Define entropy of vapourisation.

Define entropy of transition.

What are spontaneous process?

What is absolute zero temperature?

For a reaction, 2Cl_(g) ⟶ Cl₂, What are the signs of ΔH and ΔS?

In the equation N_2(g)+ 3H_2(g) ⇌2NH_3(g) What would be the sign of work done?

Which law of thermodynamics deals with equivalence of different forms of energies?

Define the following terms.

Define the term thermodynamic process.

Write the Consequence of Boyle's law.

Explain Charles' law with an experimental illustration.

Explain the graphical representation of Charles law.

Explain graphical representation of Gay Lussac's law.

Explain the graphical representation of Avogadro's hypothesis.

What is compressibility factor? How does it explain the deviation of non ideal gases from ideal behaviour.

Explain the term 'Boyle's point.' Mention is significance.

Show how the molar volume of a real and ideal gas are related to each other?

Using Andrew's isotherm of CO₂ explain the terms
(i) critical temperature
(ii) critical pressure and
(iii) critical volume.

What is inversion temperature? How is it related to Vander Waals constants?

List the uses of sodium hydroxide

Why is sodium bicarbonate nicknamed as 'Baking Soda'?

Give the uses of sodium bicarbonate

Why table salt becomes wet when kept in open space?

Why does Li₂CO₃ decompose at a temperature below 1273K?

Lithium salts are more soluble than the salts of other metals of group 1. Justify.

How does the alkali metals produce characteristic colour to the oxidising flame

Why is the density of potassium less than that of sodium?

Why are potassium and caesium, rather than lithium used in photochemical cells?

Why does lithium exhibit anomalous properties?

Mention any two biological effects of D₂O.

Name the salts that lead to the formation of permanent hardness in water can you remove permanent hardness by boiling?

How will you regenerate zeolite in ion-exchange method?