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Download Tamil Nadu 11th Standard Chemistry question papers, model tests, one-mark questions, important questions, and public exam papers in PDF format. Free study materials and answer keys for TN State Board students.

Questions:

Multiple Choice Question

216 x 1 = 216

Assertion: Helium has the highest value of ionisation energy among all the elements known
Reason: Helium has the highest value of electron affinity among all the elements known

(a)

Both assertion and reason are true and reason is correct explanation for the assertion

(b)

Both assertion and reason are true but the reason is not the correct explanation for the assertion

(c)

Assertion is true and the reason is false

(d)

Both assertion and the reason are false

Van't Hoff equation is ___________

(a)

\(\triangle G^0=-\triangle H^0-T\triangle S^0\)

(b)

G - H - TS

(c)

\(\triangle G^0\) = -2.303 RT log K_eq

(d)

\(\triangle S-\triangle H/T\)

Statement-I: Heavy water has been widely used as moderator in nuclear reactors.
Statement-II: Heavy water can lower the energies of fast moving neutrons.

(a)

Statements-I and II are correct and Statement-II is the correct explanation of statement-I.

(b)

Statements-land II are correct but Statement-II is not the correct explanation of statement-I.

(c)

Statement-I is correct but Statement-II is wrong.

(d)

Statement-I is wrong but Statement-II is correct.

Statement-I: The magnetic moment of parahydrogen is zero.
Statement-II: The spins of two hydrogen atoms in para H2 molecule neutralise each other.

(a)

Statements-I and II are correct and Statement-II is the correct explanation of statement-I.

(b)

Statements-I and II are correct but Statement-II is not the correct explanation of statement- I.

(c)

Statement-I is correct but Statement-II is wrong.

(d)

Statement-I is wrong but Statement-II is correct.

Statement-I: Hydrogen is placed at the top of the group which is in-line with the latest periodic table.
Statement-II: Hydrogen has a tendency to lose its electron to form H+, thus showing electropositive character like alkali metals. On the other hand, hydrogen has a tendency to gain an electron to yield H^-, thus showing an electronegative character like halogens.

(a)

Statements-I and II are correct and Statement-Il is the correct explanation of statement-I.

(b)

Statements-land II are correct but Statement-II is not the correct explanation of statement- I.

(c)

Statement-I is correct but Statement-II is wrong.

(d)

Statement-I is wrong but Statement-II is correct.

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

(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

Electronic configuration of species M²⁺ is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁶ and its atomic weight is 56. The number of neutrons in the nucleus of species M is ________

(a)

(b)

(c)

(d)

The equivalent mass of potassium permanganate in alkaline medium is:
MnO₄^- + 2H₂O + 3e^-\(\rightarrow\) MnO₂ + 4OH^-

(a)

31.6

(b)

52.7

(c)

(d)

None of these

Assertion: Number of radial and angular nodes for 3p orbital are 1, 1 respectively.
Reason: Number of radial and angular nodes depends only on principal quantum number.

(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

10.

Assertion: The spectrum of He⁺is expected to be similar to that of hydrogen
Reason: He⁺ is also one electron system.

(a)

If both assertion and reason are true and reason is the correct explanation of assertion.

(b)

If both assertion and reason are reason are true but reason is not the correct explanation of assertion

(c)

If assertion is true but reason is false

(d)

If both assertion and reason are false

11.

First law of thermodynamics does not give any information regarding _________

(a)

spontaneity

(b)

feasibility

(c)

both (a) & (b)

(d)

neither (a) nor (b)

12.

_________ is an intensive property

(a)

internal energy

(b)

volume

(c)

temperature

(d)

mass

13.

Identify the suitable condition(s) which helps the adiabatic process to occur?
(i) ΔT = 0
(ii)ΔP = 0
(iii) q = 0
(iv) w = 0

(a)

Only (i)

(b)

Only (iii)

(c)

(i) and (ii)

(d)

(i), (ii) and (iv)

14.

Pick out the true statement(s).
(i) q and are path functions
(ii) q + w is a state function

(a)

Only (i)

(b)

Only (ii)

(c)

Both (i) and (ii)

(d)

Both are incorrect statements

15.

For the reaction PCl5(g) ⟶ PCl_3(g) + Cl_2(g)

(a)

ΔH>ΔU

(b)

ΔH<ΔU

(c)

ΔH=ΔU

(d)

Un predictable

16.

Which of the following is a state function?

(a)

(b)

(c)

q + w

(d)

All of these

17.

The extensive and intensive properties respectively are ____________

(a)

entropy, enthalpy

(b)

entropy, temperature

(c)

enthalpy, entropy

(d)

temperature, entropy

18.

For a cyclic process involving isothermal expansion of an ideal gas.

(a)

∆U=qV

(b)

∆U=w

(c)

∆U= q + w

(d)

∆U=0

19.

In a compression process, P_ext is ___________

(a)

(P_int+ dP)

(b)

(P_int- dP)

(c)

(dP-P_int)

(d)

(-P_int+dP)

20.

The gravitational work done by an object is __________

(a)

(b)

(c)

(d)

mgh

21.

1kJ = _________J

(a)

1000

(b)

100

(c)

(d)

22.

If the heat flows out of the system into the surrounding, the q value becomes _________

(a)

+Ve

(b)

-Ve

(c)

equal to zero

(d)

maximum

23.

The SI unit of heat is ____________

(a)

Joule

(b)

Calorie

(c)

mole

(d)

J mol^-1

24.

For a cyclic process the volume of ΔU is ____________

(a)

maximum

(b)

minimum

(c)

zero

(d)

does not change

25.

Which among the following is a path function?

(a)

Enthalpy

(b)

Free energy

(c)

Internal energy

(d)

Work

26.

Which among the following is a state function?

(a)

Pressure

(b)

Enthalpy

(c)

Heat

(d)

Both (a) and (b)

27.

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

List-I	List-II
A.isochoric	1. dE = 0, dV = 0, dH = 0, dP= 0
B.cyclic	2. dT=0
C.adiabatic	3. dV=0
D.isothermal	4. q=0

(a)

A	B	C	D
3	1	4	2

(b)

A	B	C	D
1	3	4	2

(c)

A	B	C	D
3	1	2	4

(d)

A	B	C	D
1	2	3	4

28.

For an isochoric process, ΔU = _______________

(a)

(b)

q+w

(c)

q_v

(d)

29.

Internal energy is denoted by the symbol_______

(a)

(b)

(c)

(d)

30.

Which among the following is not a state function?

(a)

Pressure

(b)

Volume

(c)

Temperature

(d)

Work

31.

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

(a)

isobaric

(b)

cyclic

(c)

isothermal

(d)

isochoric

32.

For an isothermal process _____

(a)

q = 0

(b)

dV = 0

(c)

dT = 0

(d)

dP = 0

33.

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

(a)

isobaric

(b)

isothermal

(c)

adiabatic

(d)

isochoric

34.

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

(a)

isothermal

(b)

isobasic

(c)

isochoric

(d)

adiabatic

35.

All naturally occurring processes are _________ process

(a)

reversible

(b)

irreversible

(c)

cyclic process

(d)

isochoric process

36.

Which among the following is an intensive property?

(a)

free energy

(b)

heat capacity

(c)

volume

(d)

molar volume

37.

For an adiabatic process ____________

(a)

q = 0

(b)

dP = 0

(c)

dT = 0

(d)

dP = 0

38.

Which among the following is not an extensive property?

(a)

Volume

(b)

internal energy

(c)

Mass

(d)

temperature

39.

Match the list I with list II and select the answer using the code given below the list.

List-I	List-II
A. Pressure	1. intensive property
B. Number of moles	2. Path function
C. Density	3. Extensive property
D. Work	4. State function

(a)

A	B	C	D
1	2	3	4

(b)

A	B	C	D
4	3	1	2

(c)

A	B	C	D
4	3	2	1

(d)

A	B	C	D
3	4	1	2

40.

________ is an example for closed system.

(a)

Solution of CuSO4 in a beaker

(b)

A gas contained in a cylinder fitted with piston

(c)

Hot water contained in a thermos flask

(d)

Tea in a cup

41.

A portion of matter under consideration, which is separated from rest of universe by real or imaginary boundaries is called_____________

(a)

surroundings

(b)

system

(c)

boundary

(d)

Universe

42.

A fundamental goal of thermodynamics is the prediction of __________ of the process.

(a)

reversibility

(b)

rate

(c)

spontaneity

(d)

none of these

43.

The branch of science which deals the relation between energy, heat, work and accompanying changes around us is 'called' _____________

(a)

Thermodynamics

(b)

Chemical kinetics

(c)

Calorimetry

(d)

Potentiometer

44.

Electronic configuration of species M²⁺ is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁶ and its atomic weight is 56. The number of neutrons in the nucleus of species M is _______________

(a)

(b)

(c)

(d)

45.

The values of ΔH and ΔS for a reaction are respectively 30 kJ mol^-1 and 100 JK^-1 mol^-1. Then the temperature above which the reaction will become spontaneous is ______________

(a)

300 K

(b)

30 K

(c)

100 K

(d)

200 C

46.

ΔS is expected to be maximum for the reaction ____________

(a)

Ca_(S)+ 1/2O_2(g)⟶ CaO_(S)

(b)

C_(S)+O_2(g) ⟶ CO_2(g)

(c)

N_2(g)+ O_2(g)⟶ 2NO_(g)

(d)

CaCO_3(S)⟶ CaO_(S)+ CO_2(g)

47.

Molar heat of vaporization of a liquid is 4.8 kJ mol^-1. If the entropy change is 16 J mol^-1 K^-1, the boiling point of the liquid is ____________

(a)

323 K

(b)

27° C

(c)

164 K

(d)

0.3 K

48.

In an isothermal reversible compression of an ideal gas the sign of q, ΔS and w are respectively _______________

(a)

+, -, -

(b)

-, +, -

(c)

+, -, +

(d)

-, -, +

49.

The temperature of the system, decreases in an _____________

(a)

Isothermal expansion

(b)

Isothermal Compression

(c)

adiabatic expansion

(d)

adiabatic compression

50.

The correct thermodynamic conditions for the spontaneous reaction at all temperature is ______________

(a)

ΔH < 0 and ΔS > 0

(b)

ΔH < 0 and ΔS < 0

(c)

ΔH > 0 and ΔS = 0

(d)

ΔH > 0 and ΔS > 0

51.

The bond dissociation energy of methane and ethane are 360 kJ mol^-1 and 620 kJ mol^-1 respectively. Then, the bond dissociation energy of C-C bond is ______________.

(a)

170 kJ mol^-1

(b)

50 kJ mol^-1

(c)

80 kJ mol^-1

(d)

220 kJ mol^-1

52.

When 15.68 litres of a gas mixture of methane and propane are fully combusted at 0° C and 1 atmosphere, 32 litres of oxygen at the same temperature and pressure are consumed. The amount of heat of released from this combustion in KJ is _____________ (ΔH_c (CH₄) = - 890 KJ mol^-1and ΔH_c(C₃H₈ = - 2220 KJ mol^-1)

(a)

- 889 kJ mol^-1

(b)

- 1390 kJ mol^-1

(c)

- 3180 kJ mol^-1

(d)

- 635.47 kJ mol^-1

53.

Given that C_(g)+ O_2(g)⟶ CO_2(g)ΔH^o =-akJ; 2CO_(g)+O_2(g) ⟶ 2CO_2(g)ΔH^o= -bkJ; Calculate the AHo for the reaction C_(g)+ 1/2O_2(g)⟶ CO_(g) ______________

(a)

\(\frac{b+2a}{2}\)

(b)

2a-b

(c)

\(\frac{2a-b}{2}\)

(d)

\(\frac{b-2a}{2}\)

54.

The value of ΔH for cooling 2 moles of an ideal monatomic gas from 125° C to 25° C at constant pressure will be [given C_p= \(\frac{5}{2}\)R] ____________.

(a)

- 250 R

(b)

- 500 R

(c)

500 R

(d)

+ 250 R

55.

The work done by the liberated gas when 55.85 g of iron (molar mass 55.85 g mol^-1) reacts with hydrochloric acid in an open beaker at 25°C _____________

(a)

- 2.48 kJ

(b)

-2.22 kJ

(c)

+2.22 kJ

(d)

+ 2.48 kJ

56.

Change in internal energy, when 4 kJ of work is done on the system and 1 kJ of heat is given out by the system is ______________

(a)

+1 kJ

(b)

- 5 kJ

(c)

+3 kJ

(d)

- 3 kJ

57.

If one mole of ammonia and one mole of hydrogen chloride are mixed in a closed container to form ammonium chloride gas, then _____________

(a)

ΔH > ΔU

(b)

ΔH - ΔU = 0

(c)

ΔH + ΔU = 0

(d)

ΔH < ΔU

58.

Which of the following is not a thermodynamic function ?

(a)

internal energy

(b)

enthalpy

(c)

entropy

(d)

frictional energy

59.

The enthalpies of formation of Al₂O₃ and Cr₂O₃are -1596 kJ and -1134 kJ, respectively. ΔH for the reaction 2Al + Cr₂O₃ ⟶ 2Cr + Al₂O₃ is _______________

(a)

- 1365 kJ

(b)

2730 kJ

(c)

- 2730 kJ

(d)

- 462 kJ

60.

C(diamond) ) ⟶ C(graphite), ΔH = -ve, this indicates that ___________

(a)

graphite is more stable than diamond

(b)

graphite has more energy than diamond

(c)

both are equally stable

(d)

stability cannot be predicted

61.

The heat of formation of CO and CO₂ are - 26.4 kcal and - 94 kcal, respectively. Heat of combustion of carbon monoxide will be ____________

(a)

+ 26.4 kcal

(b)

- 67.6 kcal

(c)

- 120.6 kcal

(d)

+ 52.8 kcal

62.

Heat of combustion is always ____________

(a)

positive

(b)

negative

(c)

zero

(d)

either positive or negative

63.

An ideal gas expands from the volume of 1 x 10^-3 m³to 1 x 10^-2m³ at 300 K against a constant pressure at 1 x 10⁵ Nm^-2. The work done is ______________

(a)

- 900 J

(b)

900 kJ

(c)

270 kJ

(d)

-900 kJ

64.

The intensive property among the quantities below is ____________

(a)

mass

(b)

volume

(c)

enthalpy

(d)

\(\frac { mass }{ volume } \)

65.

In an adiabatic expansion of an ideal gas ____________

(a)

w = -ΔU

(b)

w = ΔU + ΔH

(c)

ΔU = O

(d)

w = 0

66.

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

(a)

> 0

(b)

> 0

(c)

< 0

(d)

= 0

67.

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

(a)

q = w

(b)

q = 0

(c)

ΔE = q

(d)

PΔV= 0

68.

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

(a)

decrease in entropy

(b)

increase in enthalpy

(c)

increase in free energy

(d)

decrease in free energy

69.

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

(a)

ΔE

(b)

ΔH

(c)

ΔS

(d)

ΔG

70.

Identify the redox reaction taking place in a beaker.

(a)

Zn_(s)+ Cu²⁺_(aq) \(\longrightarrow\) Zn²⁺_(aq) + Cu_(s)

(b)

Cu_(s) + 2Ag⁺_(aq) \(\longrightarrow\) Cu²⁺_(aq) + 2Ag_(s)

(c)

Cu_(s) + Zn²⁺_(aq) \(\longrightarrow\) Zn_(s) + Cu²⁺ _(aq)

(d)

2Ag_(s) + cu²⁺_(aq) \(\longrightarrow\) 2Ag⁺_aq + Cu_(s)

71.

In which of the following reactions, hydrogen peroxide acts as an oxidising agent?

(a)

I₂+ H₂O₂ + 20H^- \(\longrightarrow\) 21- + 2H₂O + O₂

(b)

PbS + 4H₂O₂ \(\longrightarrow\) PbSO₄ + 4H₂O

(c)

2MnO₄^-+ 3H₂O₂ \(\longrightarrow\) 2MnO₂ + 3O₂ + 2H₂O + 2OH^-

(d)

HOCI + H₂O₂ \(\longrightarrow\) H₂O⁺ + Cl^- + O₂

72.

The change in the oxidation number of S in H₂S and SO₂,in the following industrial reaction:
2H₂S_(g) + SO_2(g) \(\longrightarrow\) 3S_(s) + H2O_(g)

(a)

-2 to 0, +4 to 0

(b)

-2 to 0, +4 to -1

(c)

-2 to -1, +4 to 0

(d)

-2 to -1, +4 to -2

73.

Identify the correct statements with reference to the given reaction
P₄ + 3OH^- + 3H₂O \(\longrightarrow\) PH₃ + 3H₂PO₂^-
(i) Phosphorous is undergoing reduction only
(ii) Phosphorous is undergoing oxidation only
(iii) Phosphorous is undergoing both oxidation and reduction.
(iv) Hydrogen is undergoing neither oxidation nor reduction.

(a)

only (iii)

(b)

both (iii) and (iv)

(c)

only (i)

(d)

None of these

74.

Maximum oxidation state is present in the central metal atom of which compound

(a)

CrO₂Cl₂

(b)

MnO₂

(c)

[Fe(CN)₆]^3-

(d)

MnO

75.

25g of each of the following gases are taken at 27°C and 600 mm Hg pressure. Which of these will have the least volume?

(a)

HBr

(b)

HCI

(c)

(d)

76.

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

(a)

(b)

(c)

(d)

All of these

77.

What is the density of N₂ gas at 227^o C and 5.00 atm pressure? (R = 0.082 L atm K^-1 mol^-1 )

(a)

1.40 g/L

(b)

2.81 g/L

(c)

3.41 g/L

(d)

0.29 g/L

78.

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

(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

79.

The units of Vander Waals constants 'b' and 'a' respectively ____________

(a)

mol L^-1 and L atm² mol^-1

(b)

mol L and L atm mol²

(c)

mol^-1L and L² atm mol^-2

(d)

none of these

80.

Among the following the least thermally stable is ___________

(a)

K₂CO₃

(b)

Na₂CO₃

(c)

BaCO₃

(d)

Li₂CO₃

81.

When CaC₂ is heated in atmospheric nitrogen in an electric furnace the compound formed is ___________

(a)

Ca(CN)₂

(b)

CaNCN

(c)

CaC₂N₂

(d)

CaNC₂

82.

Formula of Gypsum is _______________

(a)

CaSO₄.2H₂O

(b)

CaSO₄·1/2 H₂O.

(c)

3CaSO₄.H₂O

(d)

2CaSO₄.2H₂O

83.

The name 'Blue John' is given to which of the following compounds ?

(a)

CaH₂

(b)

CaF₂

(c)

Ca₂(PO₄)₂

(d)

CaO

84.

Which of the following statement is false ?

(a)

Ca²⁺ ions are not important in maintaining the regular beating of the heart

(b)

Mg²⁺ ions are important in the green parts of the plants

(c)

Mg²⁺ ions form a complex with ATP

(d)

Ca²⁺ ions are important in blood clotting

85.

Which of the following does not represent the mathematical expression for the Heisenberg uncertainty principle?

(a)

\(\triangle x.\triangle p\ge \frac { h }{ 4\pi } \)

(b)

\(\triangle x.\triangle v\ge \frac { h }{ 4\pi m } \)

(c)

\(\triangle E.\triangle t\ge \frac { h }{ 4\pi } \)

(d)

\(\triangle E.\triangle x\ge \frac { h }{ 4\pi } \)

86.

Time independent Schrodinger wave equation is ______________

(a)

\(\overset { \wedge }{ H } \psi =E\psi \)

(b)

\({ \triangledown }^{ 2 }\psi +\frac { 8{ \pi }^{ 2 }m }{ { h }^{ 2 } } (E+V)\psi =0\)

(c)

\(\frac { { \partial }^{ 2 }\psi }{ { \partial x }^{ 2 } } +\frac { { \partial }^{ 2 }\psi }{ { \partial y }^{ 2 } } +\frac { { \partial }^{ 2 }\psi }{ { \partial z }^{ 2 } } +\frac { { 2m } }{ { h }^{ 2 } } (E-V)\Psi =0\)

(d)

All of these

87.

The energy of an electron in the 3rd orbit of hydrogen atom is -E. The energy of an electron in the first orbit will be ___________

(a)

-3E

(b)

\(\frac{-E}{3}\)

(c)

\(\frac{-E}{9}\)

(d)

-9E

88.

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 ____________

(a)

(b)

0.2

(c)

2.5

(d)

0.4

89.

A macroscopic particle of mass 100 g and moving at a velocity of 100 cm S^-1will have a de Broglie wavelength of ___________

(a)

6.6 x 10^-29 cm

(b)

6.6 x 10^-30 cm

(c)

6.6 x 10^-31 cm

(d)

6.6 x 10^-32 cm

90.

The compound (X) on heating gives a colourless gas and a residue that is dissolved in water to obtain (B). Excess of CO₂ is bubbled through aqueous solution of B, C is formed. Solid (C) on heating gives back X.(B) is ____________

(a)

CaCO₃

(b)

Ca(OH)₂

(c)

Na₂CO₃

(d)

NaHCO₃

91.

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 ___________

(a)

Na₂CO₃

(b)

NaHCO₃

(c)

CaCO₃

(d)

Ca(HCO₃)₂

92.

The suspension of slaked lime in water is known as ___________

(a)

lime water

(b)

quick lime

(c)

milk of lime

(d)

aqueous solution of slaked lime

93.

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

(a)

It is rendered passive by nitric acid

(b)

It forms Be₂C

(c)

Its salts are rarely hydrolysed

(d)

Its hydride is electron deficient and polymeric

94.

Which is the correct sequence of solubility of carbonates of alkaline earth metals ?

(a)

BaCO₃ > SrCO₃ > CaCO₃ > MgCO₃

(b)

MgCO₃ > CaCO₃ > SrCO₃ > BaCO₃

(c)

CaCO₃ > BaCO₃ > SrCO₃ > BaCO₃

(d)

BaCO₃ > CaCO₃ > SrCO₃ > MgCO₃

95.

Match the flame colours of the alkali and alkaline earth metal salts in the bunsen burner

(P) Sodium	(1) Brick red
(q) Calcium	(2) Yellow
(r) Barium	(3) Violet
(s) Strontium	(4) Apple green
(t) Cesium	(5) Crimsonred
(u) Potassium	(6) Blue

(a)

p - 2, q - 1, r - 4, s - 5, t - 6, u - 3

(b)

p - 1, q - 2, r - 4, s - 5, t - 6, u - 3

(c)

p - 4, q - 1, r - 2, s - 3, t - 5, u - 6

(d)

p - 6, q - 1, r - 2, s - 3, t - 5, u - 4

96.

Which of the following has highest hydration energy __________

(a)

MgCl₂

(b)

CaCl₂

(c)

BaCl₂

(d)

SrCI₂

97.

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

(a)

Ca(CN)₃

(b)

CaN₂

(c)

CaCN₂

(d)

Ca₃N₂

98.

In which process, fused sodium hydroxide is electrolysed for extraction of sodium ?

(a)

Castner's process

(b)

Cyanide process

(c)

Down process

(d)

All of these

99.

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

(a)

MF < MCI < MBr < MI

(b)

MI < MBr < MCI < MF

(c)

MI < MBr

(d)

none of these

100.

Lithium shows diagonal relationship with _____________

(a)

sodium

(b)

magnesium

(c)

calcium

(d)

aluminium

101.

Find the wrong statement

(a)

sodium metal is used in organic qualitative analysis

(b)

sodium carbonate is soluble in water and it is used in inorganic qualitative analysis

(c)

potassium carbonate can be prepared by solvay process

(d)

potassium bicarbonate is acidic salt

102.

RbO₂ is _____________

(a)

superoxide and paramagnetic

(b)

peroxide and diamagnetic

(c)

superoxide and diamagnetic

(d)

peroxide and paramagnetic

103.

sodium is stored in _____________

(a)

alcohol

(b)

water

(c)

kerosene

(d)

none of these

104.

Which of the following has the highest tendency to give the reaction \(M_{g}^{+}\xrightarrow[Medium]{Aqueous}M_{aq}^{+}\)

(a)

(b)

(c)

(d)

105.

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

(a)

ethanoic acid

(b)

ethanol

(c)

phenol

(d)

none of these

106.

Which of the following statements is in correct ?

(a)

Li⁺ has minimum degree of hydration among alkali metal cations

(b)

The oxidation state of K in KO₂ is +1

(c)

Sodium is used to make Na / Pb alloy

(d)

MgSO₄ is readily soluble in water

107.

For alkali metals, which one of the following trends is incorrect ?

(a)

Hydration energy: Li > Na > K > Rb

(b)

Ionisation energy: Li > Na > K > Rb

(c)

Density: Li < Na < K < Rb

(d)

Atomic size: Li < Na < K < Rb

108.

Maximum deviation from ideal gas is expected from ______________

(a)

CH₄(g)

(b)

NH₃ (g)

(c)

H₂(g)

(d)

N₂ (g)

109.

Four gases P, Q, R and S have almost same values of 'b' but their 'a' values (a, b are Vander Waals Constants) are in the order Q < R < S < P. At a particular temperature, among the four gases the most easily liquefiable one is __________

(a)

(b)

(c)

(d)

110.

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 ___________

(a)

(b)

1/T

(c)

(d)

none of these

111.

Equal moles of hydrogen and oxygen gases are placed in a container, with a pin-hole through which both can escape what fraction of oxygen escapes in the time required for one-half of the hydrogen to escape.

(a)

\(\frac { 3 }{ 8 } \)

(b)

\(\frac { 1 }{ 2 } \)

(c)

\(\frac { 1 }{ 8 } \)

(d)

\(\frac { 1 }{ 4 } \)

112.

At identical temperature and pressure, the rate of diffusion of hydrogen gas is 3\(\sqrt { 3 } \) times that of a hydrocarbon having molecular formula C_nH_2n-2. What is the value of n ?

(a)

(b)

(c)

(d)

113.

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

(a)

(b)

(c)

(d)

114.

Consider the following statements
i) Atmospheric pressure is less at the top of a mountain than at sea level
ii) Gases are much more compressible than solids or liquids
iii) When the atmospheric pressure increases the height of the mercury column rises.
Select the correct statement

(a)

I and II

(b)

II and III

(c)

I and III

(d)

I, II and III

115.

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

Gas	O₂	N₂	NH₃	CH₄
a	1.360	1.390	4.170	2.253

The gas which can be most easily liquefied is ______________

(a)

O₂

(b)

N₂

(c)

NH₃

(d)

CH₄

116.

Use of hot air balloon in sports at meteorological observation is an application of __________________

(a)

Boyle's law

(b)

Newton's law

(c)

Kelvin's law

(d)

Brown's law

117.

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

(a)

₆C¹²

(b)

₇C¹²

(c)

₆C¹³

(d)

₆C¹⁴

118.

Which of the following is/are true with respect to carbon -12 ?

(a)

relative atomic mass is 12 u

(b)

the oxidation number of carbon is +4 in all its compounds.

(c)

1 mole of carbon-12 contain 6.022 x 10²² carbon atoms.

(d)

All of these

119.

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

(a)

propene

(b)

ethyne

(c)

benzene

(d)

ethane

120.

Which of the following contain same number of carbon atoms as in 6 g of carbon-12 ?

(a)

7.5 g ethane

(b)

8 g methane

(c)

both (a) and (b)

(d)

none of these

121.

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 _______.

(a)

66.25 g mol^-1

(b)

44 g mol^-1

(c)

24.5 g mol^-1

(d)

662.5 g mol^-1

122.

What is the mass of precipitate formed when 50 ml of 8.5 % solution of AgNO₃ is mixed with 100 ml of 1.865 % potassium chloride solution ?

(a)

3.59 g

(b)

(c)

14 g

(d)

28 g

123.

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 ______.

(a)

Number of molecules in A and B are same

(b)

Number of molecules in B is more than that in A.

(c)

The ratio between the number of molecules in A= to number of molecules in B is 2:1

(d)

Number of molecules in B is three times greater than the number of molecules in A

124.

If Avogadro number were changed from 6.022 x 10²³to 6.022 x 10²⁰, this would change ______.

(a)

the ratio of chemical species to each other in a balanced equation

(b)

the ratio of elements to each other in a compound

(c)

the definition of mass in units of grams

(d)

the mass of one mole of carbon

125.

The equivalent mass of ferrous oxalate is __________.

(a)

\(\frac { molar\ mass\ of\ ferrous \ oxalate }{ 1 } \)

(b)

\(\frac { molar\ mass\ of\ ferrous \ oxalate }{ 2 } \)

(c)

\(\frac { molar\ mass\ of\ ferrous \ oxalate }{ 3 } \)

(d)

None of these

126.

The correct increasing order of the oxidation state of sulphur in the anions \({ SO }_{ 4 }^{ 2- },{ SO }_{ 3 }^{ 2- }{ , }{ { S }_{ 2 }{ O } }_{ 4 }^{ 2- },{ S }_{ 2 }{ O }_{ 6 }^{ 2- }\) is _________.

(a)

\({ SO }_{ 3 }^{ 2- }<{ SO }_{ 4 }^{ 2- }<{ { S }_{ 2 }{ O } }_{ 4 }^{ 2- }<{ S }_{ 2 }{ O }_{ 6 }^{ 2- }\)

(b)

\({ SO }_{ 4 }^{ 2- }<{ SO }_{ 4 }^{ 2- }<{ S }_{ 2 }{ O }_{ 6 }^{ 2- }<{ SO }_{ 3 }^{ 2- }\)

(c)

\({ { S }_{ 2 }{ O } }_{ 4 }^{ 2- }<{ SO }_{ 3 }^{ 2- }<{ S }_{ 2 }{ O }_{ 6 }^{ 2- }<{ SO }_{ 4 }^{ 2- }\)

(d)

\({ S }_{ 2 }{ O }_{ 6 }^{ 2- }<{ SO }_{ 4 }^{ 2- }<{ SO }_{ 4 }^{ 2- }<{ SO }_{ 3 }^{ 2- }\)

127.

Match the items in column list-I with relevant items in list-II.

List-I		List-II
A	Ions having positive charge	1	anion
B	Ions having negative charge	2	-1
C	Oxidation number of fluorine in NaF	3	0
D	The sum of oxidation number of all atoms in a neutral molecule	4	cation

(a)

A	B	C	D
3	4	2	1

(b)

A	B	C	D
1	2	3	4

(c)

A	B	C	D
2	3	4	1

(d)

A	B	C	D
4	1	2	3

128.

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

List-I		List-II
A	Cr₂O₇^2-	1	+5
B	MnO₄^-	2	+6
C	VO₃^-	3	+3
D	FeF₆³⁺	4	+7

(a)

A	B	C	D
3	1	4	2

(b)

A	B	C	D
4	3	2	1

(c)

A	B	C	D
2	4	1	3

(d)

A	B	C	D
3	2	1	4

129.

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

(a)

\(\frac { 1 }{ m } \sqrt { \frac { h }{ \pi } } \)

(b)

\( \sqrt { \frac { h }{ \pi } } \)

(c)

\(\frac { 1 }{ 2m } \sqrt { \frac { h }{ \pi } } \)

(d)

\( { \frac { h }{4\pi } } \)

130.

Electron density in the yz plane of 3d_xy orbital is ___________

(a)

zero

(b)

0.50

(c)

0.75

(d)

0.90

131.

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

(a)

(b)

(c)

(d)

unpredictable

132.

Consider the following sets of quantum numbers:

	n	l	m	s
(i)	3	0	0	+\(\frac { 1 }{ 2 } \)
(ii)	2	2	1	-\(\frac { 1 }{ 2 } \)
(iii)	4	3	-2	+\(\frac { 1 }{ 2 } \)
(iv)	1	0	-1	+\(\frac { 1 }{ 2 } \)
(v)	3	4	3	-\(\frac { 1 }{ 2 } \)

Which of the following sets of quantum number is not possible?

(a)

(i), (ii), (iii) and (iv)

(b)

(ii), (iv) and (v)

(c)

(i) and (iii) .

(d)

(ii), (iii) and (iv)

133.

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

(a)

ns \(\rightarrow\) (n-2)f \(\rightarrow\) (n - 1)d \(\rightarrow\) np

(b)

ns \(\rightarrow\) (n - 1) d \(\rightarrow\) (n - 2) f \(\rightarrow\) np

(c)

ns \(\rightarrow\) (n-2)f \(\rightarrow\)np \(\rightarrow\) (n-1)d

(d)

none of these are correct

134.

The total number of orbitals associated with the principal quantum number n = 3 is _________

(a)

(b)

(c)

(d)

135.

What is the maximum numbers of electrons that can be associated with the following set of quantum numbers? n = 3, I = 1 and m =-1

(a)

(b)

(c)

(d)

= 10

136.

Identify the correct statement(s) with respect to the following reaction :
Zn + 2HCl \(\longrightarrow\) ZnCl₂ + H₂
(i) Zinc is acting as an oxidant
(ii) Chlorine is acting as a reductant
(iii) Hydrogen is not acting as an oxidant
(iv) Zn is acting as a reductant

(a)

only (ii)

(b)

only (iv)

(c)

both (ii) and (iii)

(d)

both (ii) and (i)

137.

Which of the following statement(s) is/are not true about the following decomposition reaction.
2KClO₃ \(\longrightarrow\) 2KCl + 3O₂
(i) Potassium is undergoing oxidation
(ii) Chlorine is undergoing oxidation
(iii) Oxygen is reduced
(iv) None of the species are undergoing oxidation and reduction.

(a)

only (iv)

(b)

(i) and (iv)

(c)

(iv) and (iii)

(d)

All of these

138.

Identify disproportionation reaction

(a)

CH₄ + 2O₂ \(\longrightarrow\) CO₂+ 2H₂O

(b)

CH₄ + 4Cl₂ \(\longrightarrow\) CCl₄ + 4HCI

(c)

2F₂+ 2OH \(\longrightarrow\) 2F^-+ OF₂+ H₂O

(d)

2NO₂ + 2OH^- \(\longrightarrow\) NO^-₂ + NO^-₃ + H₂O

139.

Rusting of iron articles is an example of ___________ reaction

(a)

Combustion

(b)

decomposition

(c)

redox

(d)

hydrolysis

140.

Consider the following statements :
(i) Oxidation number of He = zero
(ii) Increase in oxidation number results in reduction.
(iii) The substance undergoing the increase in oxidation number is reducing agent.
Which among the above statement(s) is/are correct?

(a)

only (i)

(b)

(ii) and (iii)

(c)

(i) and (iii)

(d)

only (ii)

141.

Among the three metals, zinc, copper and silver, the electron releasing tendency decreases in the following order.

(a)

zinc > silver > copper

(b)

zinc > copper > silver

(c)

silver > copper > zinc

(d)

copper > silver > zinc

142.

The oxidation number of Cr in Cr₂O₇^2- _______ is

(a)

(b)

-6

(c)

(d)

-7

143.

The value of the gas constant R is ____________

(a)

0.082 dm³ atm.

(b)

0.987 cal mol^-1K^-1

(c)

8.3 J mol^-1 K^-1

(d)

8 erg mol^-1 K^-1

144.

The value of universal gas constant depends upon __________

(a)

Temperature of the gas

(b)

Volume of the gas

(c)

Number of moles of the gas

(d)

units of Pressure and volume.

145.

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 ___________

(a)

At the center of the tube

(b)

Near the hydrogen chloride bottle

(c)

Near the ammonia bottle

(d)

Throughout the length of the tube

146.

The temperatures at which real gases obey the ideal gas laws over a wide range of pressure is called ____________-

(a)

Critical temperature

(b)

Boyle temperature

(c)

Inversion temperature

(d)

Reduced temperature

147.

Equal weights of methane and oxygen are mixed in an empty container at 298 K. The fraction of total pressure exerted by oxygen is ___________

(a)

\(\frac { 1 }{ 3 } \)

(b)

\(\frac { 1 }{ 2 } \)

(c)

\(\frac { 2 }{ 3 } \)

(d)

\(\frac { 1 }{ 3 } \times 273\times 298\)

148.

When an ideal gas undergoes unrestrained expansion, no cooling occurs because the molecules _____________

(a)

are above inversion temperature

(b)

exert no attractive forces on each other

(c)

do work equal to the loss in kinetic energy

(d)

collide without loss of energy

149.

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)

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

150.

Rate of diffusion of a gas is ________

(a)

directly proportional to its density

(b)

directly proportional to its molecular weight

(c)

directly proportional to its square root of its molecular weight

(d)

inversely proportional to the square root of its molecular weight

151.

Gases deviate from ideal behavior at high pressure. Which of the following statement(s) is correct for non-ideality?

(a)

at high pressure the collision between the gas molecule become enormous

(b)

at high pressure the gas molecules move only in one direction

(c)

at high pressure, the volume of gas become insignificant

(d)

at high pressure the intermolecular interactions become significant

152.

Total number of electrons present in 1.7 g of ammonia is _____.

(a)

6.022\(\times\)10²³

(b)

\(\frac { 6.022\times { 10 }^{ 22 } }{ 1.7 } \quad \)

(c)

\(\frac { 6.022\times { 10 }^{ 24 } }{ 1.7 } \)

(d)

\(\frac { 6.022\times { 10 }^{ 23 } }{ 1.7 } \)

153.

7.5 g of a gas occupies a volume of 5.6 litres at 0° C and 1 atm pressure. The gas is ________.

(a)

(b)

N₂O

(c)

(d)

CO₂

154.

Which one of the following represents 180 g of water ?

(a)

5 Moles of water

(b)

90 moles of water

(c)

\(\frac { 6.022\times { 10 }^{ 23 } }{ 180 } \) molecules of water

(d)

6.022\(\times\)10²⁴molecules of water

155.

Which of the following pairs of elements exhibit diagonal relationship?

(a)

Be and Mg

(b)

Li and Mg

(c)

Be and B

(d)

Be and Al

156.

How does electron affinity change when we move from left to right in a period in the periodic table?

(a)

Generally increases

(b)

Generally decreases

(c)

Remains unchanged

(d)

First increases and then decreases

157.

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?

(a)

Decreases in a period and increases along the group

(b)

Increases in a period and decreases in a group

(c)

Increases both in the period and the group

(d)

Decreases both in the period and in the group

158.

The First ionisation potential of Na, Mg and Si are 496, 737 and 786 kJ mol^-1 respectively. The ionisation potential of Al will be closer to

(a)

760 kJ mol^-1

(b)

575 kJ mol^-1

(c)

801 kJ mol^-1

(d)

419 kJ mol^-1

159.

Which of the following orders of ionic radii is correct

(a)

H^- > H⁺ > H

(b)

Na⁺ > F^-> O^2-

(c)

F > O^2- > Na⁺

(d)

None of these

160.

In a given shell the order of screening effect is

(a)

s > p > d > f

(b)

s > p > f > d

(c)

f > d > p > s

(d)

f > p > s > d

161.

lE₁ and IE₂ of Mg are 179 and 348 kcal mol^-1 respectively. The energy required for the reaction Mg ⟶Mg²⁺+2e^- is

(a)

+169 kcal mol^-1

(b)

-169 kcal mol^-1

(c)

+ 527 kcal mol^-1

(d)

-527 kcal mol^-1

162.

Which of the following is second most electronegative element?

(a)

Chlorine

(b)

Fluorine

(c)

Oxygen

(d)

Sulphur

163.

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

(a)

1s₂, 2s₂, 2p⁶ 3s¹

(b)

1s², 2s²,2p⁶, 3s²

(c)

1s², 2s²,2p⁶, 3s², 3s², 3p⁶, 4s¹

(d)

Is², 2s²,2p⁶, 3s², 3p¹

164.

The correct order of decreasing electronegativity values among the elements X, Y, Z and A with atomic numbers 4, 8,7 and 12 respectively

(a)

Y > Z > X > A

(b)

Z > A >Y > X

(c)

X > Y > Z > A

(d)

X > Y > A > Z

165.

The element with positive electron gain enthalpy is

(a)

Hydrogen

(b)

Sodium

(c)

Argon

(d)

Fluorine

166.

Which one of the following is the least electronegative element?

(a)

Bromine

(b)

Chlorine

(c)

Iodine

(d)

Hydrogen

167.

Choose the disproportionation reaction among the following redox reactions.

(a)

3Mg_(s) + N_2(g) \(\longrightarrow \) Mg₃N_2(s)

(b)

P₄(s) + 3NaOH + 3H₂O \(\longrightarrow \) PH ₃(g) + 3NaH₂ PO₂(aq)

(c)

Cl_2(g) + 2Kl_(aq) \(\longrightarrow \) 2KCl_{(aq) +}I₂

(d)

Cr₂O_3(s) + 2A1_(s) \(\longrightarrow \) Al₂O₃(s) + 2Cr(s)

168.

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

(a)

Cu + 2H₂SO₄ \(\longrightarrow \) CuSO₄ +SO₂ + 2H₂O

(b)

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

(c)

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

(d)

None of the above

169.

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 ______.

(a)

2 moles of HCl (g)

(b)

0.5 moles of HCl (g)

(c)

1.5 moles of HCl (g)

(d)

1 moles of HCl (g)

170.

When 6.3 g of sodium bicarbonate is added to 30 g of the acetic acid solution, the residual solution is found to weigh 33 g. The number of moles of carbon dioxide released in the reaction is _____.

(a)

(b)

0.75

(c)

0.075

(d)

0.3

171.

For d-electron, the orbital angular momentum is ___________

(a)

\(\frac { \sqrt { 2 } h }{ 2\pi } \)

(b)

\(\\ \frac { \sqrt { 2h } }{ 2\pi } \)

(c)

\(\frac { \sqrt { 2\times 4 } h }{ 2\pi } \)

(d)

\(\frac { \sqrt { 6 } h }{ 2\pi } \)

172.

The maximum number of electrons in a sub shell is given by the expression _____________

(a)

2n²

(b)

2l + 1

(c)

4l + 2

(d)

none of these

173.

Two electrons occupying the same orbital are distinguished by ___________

(a)

azimuthal quantum number

(b)

spin quantum number

(c)

magnetic quantum number

(d)

orbital quantum number

174.

Based on equation E = \(-2.178\times { 10 }^{ -18 }J\left( \frac { { Z }^{ 2 } }{ { n }^{ 2 } } \right) \)certain conclusions are written. Which of them is not correct?

(a)

Equation can be used to calculate the change in energy when the electron changes orbit

(b)

For n = 1, the electron has a more negative energy than it does for n = 6 which means that the electron is more loosely bound in the smallest allowed orbit

(c)

The negative sign in equation simply means that the energy of electron bound to the nucleus is lower than it would be if the electrons were at the infinite distance from the nucleus.

(d)

Larger the value of n, the larger is the orbit radius.

175.

The electronic configuration of Eu (Atomic no. 63) Gd (Atomic no. 64) and Tb (Atomic no. 65) are ____________

(a)

[Xe] 4f⁶ 5d¹ 6s², [Xe] 4f⁷ Sd¹ 6s² and [Xe] 4f⁸5d¹ 6s²

(b)

[Xe] 4f⁷ , 6s², [Xe] 4f⁷ 5d¹ 6s² and [Xe] 4f⁹ 6s²

(c)

[Xe] 4f⁷ ,6s², [Xe] 4f⁸ 6s² and [Xe] 4f⁸ 5d¹ 6s²

(d)

[Xe] 4f⁶5d¹ 6s², [Xe] 4f⁷ 5d¹ 6s² and [Xe] 4f⁹ 6s²

176.

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

177.

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

(a)

n = 6 to n = 1

(b)

n = 5 to n = 4

(c)

n = 5 to n = 3

(d)

n = 6 to n = 5

178.

Water is a ___________

(a)

basic oxide

(b)

acidic oxide

(c)

amphoteric oxide

(d)

none of these

179.

Heavy water is used as _________

(a)

moderator in nuclear reactions

(b)

coolant in nuclear reactions

(c)

both (a) and (b)

(d)

none of these

180.

The type of H-bonding present in ortho nitro phenol and p-nitro phenol are respectively ____________

(a)

inter molecular H-bonding and intra molecular H-bonding

(b)

intra molecular H-bonding and inter molecular H-bonding

(c)

intra molecular H - bonding and no H - bonding

(d)

intra molecular H - bonding and intra molecular H - bonding

181.

In solid ice, oxygen atom is surrounded _____________

(a)

tetrahedrally by 4 hydrogen atoms

(b)

octahedrally by 2 oxygen and 4 hydrogen atoms

(c)

tetrahedrally by 2 hydrogen and 2 oxygen atoms

(d)

octahedrally by 6 hydrogen atoms

182.

The reaction H₃PO₂ + D₂O ➝ H₂DPO₂ + HDO indicates that hypo-phosphorus acid is _____________

(a)

tribasic acid

(b)

dibasic acid

(c)

mono basic acid

(d)

none of these

183.

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

(a)

sp and Sp³

(b)

sp and sp

(c)

Sp and Sp²

(d)

Sp³and Sp³

184.

Volume strength of 1.5 N H₂O₂ is _____________

(a)

1.5

(b)

4.5

(c)

16.8

(d)

8.4

185.

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

(a)

\(\frac{1}{2}\)

(b)

\(\frac{3}{2}\)

(c)

\(\frac{5}{2}\)

(d)

\(\frac{7}{2}\)

186.

When hydrogen peroxide is shaken with an acidified solution of potassium dichromate in presence of ether, the ethereal layer turns blue due to the formation of _____________

(a)

Cr₂O₃

(b)

\({ CrO }_{ 4 }^{ 2- }\)

(c)

CrO(O₂)₂

(d)

none of these

187.

A commercial sample of hydrogen peroxide marked as 100 volume H₂O₂, it means that _____________

(a)

1 ml of H₂O₂ will give 100 ml O₂ at STP

(b)

1 L of H₂O₂ will give 100 ml O₂ at STP

(c)

1 L of H₂O₂ will give 22.4 L O₂

(d)

1 ml of H₂O₂ will give 1 mole of O₂ at STP

188.

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

189.

The cause of permanent hardness of water is due to _____________

(a)

Ca(HCO₃)₂

(b)

Mg(HCO₃)₂

(c)

CaCl₂

(d)

MgCO₃

190.

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

(a)

sodium thio sulphate

(b)

potassium permanganate

(c)

hydrogen peroxide

(d)

EDTA

191.

If a body of a fish contains 1.2 g hydrogen in its total body mass, if all the hydrogen is replaced with deuterium then the increase in body weight of the fish will be ______________

(a)

1.2 g

(b)

2.4 g

(c)

3.6 g

(d)

\(\sqrt{4.8}\)g

192.

Non-stoichiometric hydrides are formed by _____________

(a)

palladium, vanadium

(b)

carbon, nickel

(c)

manganese, lithium

(d)

nitrogen, chlorine

193.

Tritium nucleus contains _____________

(a)

1 p+0 n

(b)

2 p+1 n

(c)

1 p + 2 n

(d)

none of these

194.

Ionic hydrides are formed by _____________

(a)

halogens

(b)

halogens

(c)

inert gases

(d)

group one elements

195.

Which one of the following statements is incorrect with regard to ortho and para dihydrogen ?

(a)

They are nuclear spin isomers

(b)

Ortho isomer has zero nuclear spin whereas the para isomer has one nuclear spin

(c)

The para isomer is favoured at low temperatures

(d)

The thermal conductivity of the para isomer is 50% greater than that of the ortho isomer

196.

Water gas is _____.

(a)

H₂O_(g)

(b)

CO + H₂O

(c)

CO + H₂

(d)

CO + N₂

197.

Which of the following statements about hydrogen is incorrect?

(a)

Hydrogen ion, H₃O⁺ exists freely in solution.

(b)

Dihydrogen acts as a reducing agent.

(c)

Hydrogen has three isotopes of which tritium is the most common.

(d)

Hydrogen never acts as cation in ionic salts.

198.

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

(a)

I > Br > CI > F

(b)

F > CI > Br > I

(c)

CI > F > Br > I

(d)

Br > I> CI > F

199.

Which one of the following arrangements represent the correct order of least negative to most negative electron gain enthalpy

(a)

Al < O < C < Ca < F

(b)

Al < Ca < O < C

(c)

C < F < O < Al < Ca

(d)

Ca < Al < C < O < F

200.

Identify the wrong statement.

(a)

Amongst the isoelectronic species, smaller the positive charge on cation, smaller is the ionic radius

(b)

Amongst isoelectric species greater the negative charge on the anion, larger is the ionic radius

(c)

Atomic radius of the elements increases as one moves down the first group of the periodic table

(d)

Atomic radius of the elements decreases as one moves across from left to right in the 2nd period of the periodic table

201.

In the third period the first ionization potential is of the order

(a)

Na > Al > Mg > Si > P

(b)

Na< Al < Mg < Si < P

(c)

Mg > Na > Si > P > Al

(d)

Na < Al < Mg < Si < P

202.

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

IE₁	IE₂	IE₃	IE₄	IE₅
577.5	1,810	2,750	11,580	14,820

The element is

(a)

phosphorus

(b)

Sodium

(c)

Aluminium

(d)

Silicon

203.

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

(a)

Chlorine

(b)

Nitrogen

(c)

Cesium

(d)

Fluorine

204.

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)

205.

The group of elements in which the differentiating electron enters the anti penultimate shell of atoms are called ___________

(a)

p-block elements

(b)

d-block elements

(c)

s-block elements

(d)

f-block elements

206.

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 ___________

(a)

(b)

AB₂

(c)

A₂B

(d)

none of the above

207.

What would be the IUPAC name for an element with atomic number 222?

(a)

bibibiium

(b)

bididium

(c)

didibium

(d)

bibibium

208.

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 ______________.

(a)

(b)

4.4%

(c)

16%

(d)

8.4%

209.

The number of water molecules in a drop of water weighing 0.018 g is ________.

(a)

6.022\(\times\)10²⁶

(b)

6.022\(\times\)10²³

(c)

6.022\(\times\)10²⁰

(d)

9.9 \(\times\)10²²

210.

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

(a)

102 g

(b)

27 g

(c)

270 g

(d)

78 g

211.

Carbon forms two oxides, namely carbon monoxide and carbon dioxide. The equivalent mass of which element remains constant ?

(a)

Carbon

(b)

Oxygen

(c)

Both carbon and oxygen

(d)

Neither carbon nor oxygen

212.

An element X has the following isotopic Composition ²⁰⁰X = 90%, ¹⁹⁹X = 8% and ²⁰²X=2%.The Weighted average atomic mass of the element X is closest to _________.

(a)

201 u

(b)

202 u

(c)

199 u

(d)

200 u

213.

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 _______.

(a)

40 ml CO₂ gas

(b)

40 ml CO₂ gas and 80 ml H₂O gas

(c)

60 ml CO₂ gas and 60 ml H₂O gas

(d)

120 ml CO₂ gas

214.

Splitting of spectral lines in an electric field is called _____________

(a)

Zeeman effect

(b)

Shielding effect

(c)

Compton effect

(d)

Stark effect

215.

The energies E₁and E₂ of two radiations are 25 eV and 50 eV respectively. The relation between their wavelengths ie \(\lambda \)₁ and\(\lambda \)₂ will be ___________

(a)

\(\frac { { \lambda }_{ 1 } }{ { \lambda }_{ 2 } } =1\)

(b)

\({ \lambda }_{ 1 }=2{ \lambda }_{ 2 }\)

(c)

\({ \lambda }_{ 1 }=\sqrt { 25\times 50{ \lambda }_{ 2 } } \)

(d)

\(2{ \lambda }_{ 1 }={ \lambda }_{ 2 }\)

216.

The energy of light of wavelength 45 nm is _____________.

(a)

6.67 x 10¹⁵J

(b)

6.67 x 10¹¹J

(c)

4.42 x 10^-18J

(d)

4.42 x 10^-15J

Assertion and reason

5 x 2 = 10

217.

Assertion (A): In the reaction between potassium permanganate and potassium iodide, permanganate ions act as oxidising agent.
Reason (R): Oxidation state of manganese changes from +2 to +7 during the reaction.
Codes:
(a) Both A and R are true and R explains A
(b) Both A and R are true but R does not explain A
(c) A is true but R is false
(d) Both A and R are false

(a)

Both A and R are true and R explains A

(b)

Both A and R are true but R does not explain A

(c)

A is true but R is false

(d)

Both A and R are false

218.

Assertion (A): Among halogens fluorine is the best oxidant.
Reason (R): Fluorine is the most electronegative atom.
Codes:
(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

(a)

Both A and R are true and R explains A

(b)

Both A and R are true but R does not explain A

(c)

A is true but R is false

(d)

Both A and R are false

219.

Assertion : BeSO₄ is soluble in water while BaSO₄ is not
Reason : Hydration energy decreases down the group from Be to Ba and lattice energy remains almost constant.
(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) both assertion and reason are false.
(d) Both assertion and reason are false

(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.

220.

Assertion : Generally alkali and alkaline earth metals form superoxides
Reason : There is a single bond between O and O in superoxides
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

(a)

both assertion and reason are true and reason 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

221.

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

(a)

both assertion and reason are true and the reason is the correct explanation of assertion

(b)

both assertion and reason are true but the reason is not the correct explanation of assertion

(c)

an assertion is true but reason is false

(d)

both assertion and reason are false

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Answers Key:

Multiple Choice Question

216 x 1 = 216

(a)
Statements-I and II are correct and Statement-II is the correct explanation of statement-I.

(a)
Statements-I and II are correct and Statement-II is the correct explanation of statement-I.

(a)
Statements-I and II are correct and Statement-Il is the correct explanation of statement-I.

(a)
Both assertion and reason are true and reason is the correct explanation of assertion.

(b)
52.7

10.

(a)
If both assertion and reason are true and reason is the correct explanation of assertion.

11.

12.

13.

(b)
Only (iii)

14.

15.

(a)
ΔH>ΔU

16.

17.

(b)
entropy, temperature

18.

(a)
∆U=qV

19.

(a)
(P_int+ dP)

20.

(d)
mgh

21.

(a)
1000

22.

(b)
-Ve

23.

(a)
Joule

24.

25.

(d)
Work

26.

(d)
Both (a) and (b)

27.

(a)

A B C D

3 1 4 2

28.

29.

(d)
U

30.

(d)
Work

31.

(d)
isochoric

32.

33.

(b)
isothermal

34.

(d)
adiabatic

35.

(b)
irreversible

36.

(d)
molar volume

37.

(a)
q = 0

38.

(d)
temperature

39.

(b)

A B C D

4 3 1 2

40.

(b)
A gas contained in a cylinder fitted with piston

41.

(b)
system

42.

43.

(a)
Thermodynamics

44.

45.

(a)
300 K

46.

(d)
CaCO_3(S)⟶ CaO_(S)+ CO_2(g)

47.

(b)
27° C

48.

(d)
-, -, +

49.

50.

(a)
ΔH < 0 and ΔS > 0

51.

52.

(d)
- 635.47 kJ mol^-1

53.

(d)
\(\frac{b-2a}{2}\)

54.

(b)
- 500 R

55.

(a)
- 2.48 kJ

56.

57.

(d)
ΔH < ΔU

58.

(d)
frictional energy

59.

(d)
- 462 kJ

60.

(a)
graphite is more stable than diamond

61.

(b)
- 67.6 kcal

62.

(b)
negative

63.

(a)
- 900 J

64.

(d)
\(\frac { mass }{ volume } \)

65.

(a)
w = -ΔU

66.

(d)
= 0

67.

(b)
q = 0

68.

(d)
decrease in free energy

69.

(b)
ΔH

70.

(d)
2Ag_(s) + cu²⁺_(aq) \(\longrightarrow\) 2Ag⁺_aq + Cu_(s)

71.

(b)
PbS + 4H₂O₂ \(\longrightarrow\) PbSO₄ + 4H₂O

72.

(a)
-2 to 0, +4 to 0

73.

(b)
both (iii) and (iv)

74.

(a)
CrO₂Cl₂

75.

(d)
HI

76.

77.

78.

(d)
both assertion and reason are false

79.

80.

(d)
Li₂CO₃

81.

(b)
CaNCN

82.

(a)
CaSO₄.2H₂O

83.

(b)
CaF₂

84.

(a)
Ca²⁺ ions are not important in maintaining the regular beating of the heart

85.

(d)
\(\triangle E.\triangle x\ge \frac { h }{ 4\pi } \)

86.

(a)
\(\overset { \wedge }{ H } \psi =E\psi \)

87.

(d)
-9E

88.

(d)
0.4

89.

90.

(b)
Ca(OH)₂

91.

(b)
NaHCO₃

92.

93.

94.

(b)
MgCO₃ > CaCO₃ > SrCO₃ > BaCO₃

95.

(a)
p - 2, q - 1, r - 4, s - 5, t - 6, u - 3

96.

(a)
MgCl₂

97.

98.

(a)
Castner's process

99.

(b)
MI < MBr < MCI < MF

100.

(b)
magnesium

101.

102.

(a)
superoxide and paramagnetic

103.

104.

(b)
Li

105.

(d)
none of these

106.

(a)
Li⁺ has minimum degree of hydration among alkali metal cations

107.

108.

(b)
NH₃ (g)

109.

(a)
P

110.

(b)
1/T

111.

112.

(b)
4

113.

114.

(d)
I, II and III

115.

116.

(a)
Boyle's law

117.

(a)
₆C¹²

118.

(a)
relative atomic mass is 12 u

119.

(a)
propene

120.

121.

(b)
44 g mol^-1

122.

(a)
3.59 g

123.

124.

(d)
the mass of one mole of carbon

125.

126.

127.

(d)

A B C D

4 1 2 3

128.

129.

130.

(a)
zero

131.

(b)
17

132.

(b)
(ii), (iv) and (v)

133.

(a)
ns \(\rightarrow\) (n-2)f \(\rightarrow\) (n - 1)d \(\rightarrow\) np

134.

(a)
9

135.

136.

(b)
only (iv)

137.

(b)
(i) and (iv)

138.

(d)
2NO₂ + 2OH^- \(\longrightarrow\) NO^-₂ + NO^-₃ + H₂O

139.

140.

141.

(b)
zinc > copper > silver

142.

(a)
+6

143.

144.

(d)
units of Pressure and volume.

145.

(b)
Near the hydrogen chloride bottle

146.

(b)
Boyle temperature

147.

(a)
\(\frac { 1 }{ 3 } \)

148.

(b)
exert no attractive forces on each other

149.

150.

(d)
inversely proportional to the square root of its molecular weight

151.

(d)
at high pressure the intermolecular interactions become significant

152.

(a)
6.022\(\times\)10²³

153.

(a)
NO

154.

(d)
6.022\(\times\)10²⁴molecules of water

155.

(d)
Be and Al

156.

(a)
Generally increases

157.

(a)
Decreases in a period and increases along the group

158.

(b)
575 kJ mol^-1

159.

(d)
None of these

160.

(a)
s > p > d > f

161.

162.

(a)
Chlorine

163.

(a)
1s₂, 2s₂, 2p⁶ 3s¹

164.

(a)
Y > Z > X > A

165.

166.

(d)
Hydrogen

167.

(b)
P₄(s) + 3NaOH + 3H₂O \(\longrightarrow \) PH ₃(g) + 3NaH₂ PO₂(aq)

168.

169.

(d)
1 moles of HCl (g)

170.

171.

(d)
\(\frac { \sqrt { 6 } h }{ 2\pi } \)

172.

173.

(b)
spin quantum number

174.

(b)
For n = 1, the electron has a more negative energy than it does for n = 6 which means that the electron is more loosely bound in the smallest allowed orbit

175.