Hot concentrated sulphuric acid is a moderately strong oxidizing agent. Which of the following reactions does not show oxidising behaviour ?

(a)

Cu + 2H₂ SO₄ \(\longrightarrow \) CuSO₄ +SO₂ + 2H₂O

(b)

C + 2H₂ + SO₄ \(\longrightarrow \) CO₂ + 2SO₂ + 2H₂O

(c)

BaCl₂ + H₂SO₄ \(\longrightarrow \) BaSO₄ + 2HCl

(d)

None of the above

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

(a)

d_z2, d_xz

(b)

d_xz, d_yZ

(c)

d_z2, d_x²-y²

(d)

d_xy ,d_x^2-y²

The value of Bohr radius for hydrogen atom is ___________

(a)

0.529 \(\times\) 10^-8 cm

(b)

0.529 \(\times\) 10^-10 cm

(c)

0.529 \(\times\) 10^-12 cm

(d)

0.529 \(\times\) 10^-12 cm

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

(a)

I< Br < CI < F (increasing electron gain enthalpy)

(b)

Li < Na < K < Rb (increasing metallic radius)

(c)

Al³⁺< Mg²⁺ < Na⁺ - (increasing ionic size)

(d)

B < C < O < N (increasing first ionisation enthalpy)

The highest ionization energy is exhibited by_________

(a)

halogens

(b)

alkaline earth metals

(c)

transition metals

(d)

noble gases

Zeolite used to soften hardness of water is hydrated _____________

(a)

Sodium aluminium silicate

(b)

Calcium aluminium silicate

(c)

Zinc aluminium borate

(d)

Lithium aluminium hydride

Among the following the least thermally stable is ___________

(a)

K₂CO₃

(b)

Na₂CO₃

(c)

BaCO₃

(d)

Li₂CO₃

Which of the following is the correct expression for the equation of state of van der Waals gas?

(a)

\(\left( P+\frac { a }{ { n }^{ 2 }{ V }^{ 2 } } \right) (V-nb)=nRT\)

(b)

\(\left( P+\frac { na }{ { n }^{ 2 }{ V }^{ 2 } } \right) (V-nb)=nRT\)

(c)

\(\left( P+\frac { { an }^{ 2 } }{ { V }^{ 2 } } \right) (V-nb)=nRT\)

(d)

\(\left( \frac { P+{ n }^{ 2 }{ a }^{ 2 } }{ { V }^{ 2 } } \right) (V-ab)=nRT\)

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

(a)

ΔE

(b)

ΔH

(c)

ΔS

(d)

ΔG

Two similar reactions are given below:
H₂(g)+\(\frac { 1 }{ 2 } \)O₂(g) \(\rightarrow\)H₂O(g); \(\Delta\)H = \(\Delta\)H₁
H₂(g)+\(\frac { 1 }{ 2 } \)O₂(g)\(\rightarrow\)H₂O(l); \(\Delta\)H =  \(\Delta\)H₂
In terms of magnitude, of \(\Delta\)H

(a)

\(\Delta\)H₁ > \(\Delta\)H₂

(b)

\(\Delta\)H₁ < \(\Delta\)H₂

(c)

\(\Delta\)H₁ = \(\Delta\)H₂

(d)

cannot be predicted

Solubility of carbon dioxide gas in cold water can be increased by ____________

(a)

increase in pressure

(b)

decrease in pressure

(c)

increase in volume

(d)

none of these

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 __________

(a)

\(1/K_1\)

(b)

\(K_1^2\)

(c)

\(({1\over K_1})^{1/2}\)

(d)

\({K_1\over 2}\)

At 100^o C the vapour pressure of a solution containing 6.5g a solute in 100g water is 732mm. If K_b = 0.52, the boiling point of this solution will be __________

(a)

102^oC

(b)

100^oC

(c)

101^oC

(d)

100.52^oC

Structure of the compound whose IUPAC name is 5,6 - dimethylhept - 2 - ene is ___________

(a)

(b)

(c)

(d)

None of these

An alkyl bromide (A) reacts with sodium in ether to form 4, 5– diethyloctane, the compound (A) is _________

(a)

CH₃ (CH₂)₃ Br

(b)

CH₃(CH₂)₅ Br

(c)

CH₃(CH₂)₃ CH(Br)CH₃

(d)

\({ CH }_{ 3 }-{ \left( { CH }_{ 2 } \right) }_{ 2 }-CH\left( Br \right) -\underset { \overset { { | } }{ { CH }_{ 3 } } }{ { CH }_{ 2 } } \)

How many orbitals are possible for n = 4?

Discuss the three types of Covalent hydrides.

State charles law and give an example.

At 0°C, ice and water are in equilibrium and the enthalpy change for the process, H₂O(s) \(\rightleftharpoons \) H₂O(l) is 6 KJ mol^-1 Calculate the entropy change for the conversion ice into water.

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

Write a note on homologous series.

Explain inductive effect with suitable example.

Describe the mechanism of Nitration of benzene.

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

What mass of N₂ will be required to produce 34g of NH₃ by the reaction, N₂ + 3H₂ \(\longrightarrow\) 2NH₃·

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

Give a brief account of the shapes of atomic orbitals?

The second electron affinity of O is positive, whereas first is negative. Give reason.

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

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.

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

Write structural formula for the following compounds
m - dinitrobenzene
 

An organic compound (A) with molecular formula C₂H₅Cl reacts with KOH gives compounds (B) and with alcoholic KOH gives compound (C). Identify (A),(B), and (C)

1. 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

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

1. List out and compare the chemical properties of metals and non-metals.

2. Compare the structures of H₂O and H₂O₂ .

1. A 10 L cylinder consist of mixture of helium, oxygen, and nitrogen of masses 0.4 g, 1.6 g and 1.4 g at 27°C. Calculate the partial pressures of He, O and N and finally arrive at the total pressure. Assume the gases to behave ideally.

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

1. The atmospheric oxidation of NO
   2NO(g) + O₂(g) ⇌ 2NO₂(g)
   was studied with initial pressure of 1 atm of NO and 1 atm of O₂. At equilibrium, partial pressure of oxygen is 0.52 atm calculate K_p of the reaction.

2. A sample of 12 M Concentrated hydrochloric acid has a density 1.2 gL^–1 Calculate the molality.

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

2. Give IUPAC names for the following compounds
   CH₃ – CH = CH – CH = CH – C ≡ C – CH₃