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

(a)

> 0

(b)

> 0

(c)

< 0

(d)

= 0

The intensive property among the quantities below is ____________

(a)

mass

(b)

volume

(c)

enthalpy

(d)

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

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

(a)

- 1365 kJ

(b)

2730 kJ

(c)

- 2730 kJ

(d)

- 462 kJ

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

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^-1 and 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

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)

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

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

(a)

isobaric

(b)

isothermal

(c)

adiabatic

(d)

isochoric

Internal energy is denoted by the symbol_______

(a)

H

(b)

S

(c)

G

(d)

U

Which among the following is a state function?

(a)

Pressure

(b)

Enthalpy

(c)

Heat

(d)

Both (a) and (b)

Which among the following is a path function?

(a)

Enthalpy

(b)

Free energy

(c)

Internal energy

(d)

Work

The SI unit of heat is ____________

(a)

Joule

(b)

Calorie

(c)

mole

(d)

J mol^-1

The gravitational work done by an object is __________

(a)

Qv

(b)

fx

(c)

PV

(d)

mgh

In a compression process, P_ext is ___________

(a)

(P_int+ dP)

(b)

(P_int- dP)

(c)

(dP-P_int)

(d)

(-P_int+dP)

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)

The heat of neutralisation of strong acid and strong base is __________

(a)

+57.32 KJ

(b)

+75.32 KJ

(c)

-75.32 KJ

(d)

-57.32 KJ

In an exothermic reaction, heat is evolved and system loses heat to the surroundings. For such system
(i) q_p will be negative
(ii) Δ_rH will be positive
(iii) q_p  will be positive
(iv) Δ_rH will be negative

(a)

(i), (ii)

(b)

(iii), (iv)

(c)

(i) & (iv)

(d)

(ii) & (iii)

For a given reaction \(\triangle\)G obtained was having positive sign convention. State whether the reaction was spontaneous or non-spontaneous.

(a)

spontaneous

(b)

non-spontaneous

(c)

reversible

(d)

equilibrium

The condition for standard free energy is _______

(a)

298 K, 1 atm

(b)

273 K, 1 atm

(c)

298⁰ C, 5 atm

(d)

25 K, 1atm

Solve: ΔH=10 k cal mol^-1, ΔS=20 cal deg^-1 mol^-1 and T=300k. Then ΔG=?

(a)

-18,000 cals mol^-1

(b)

18,000 cals mol^-1

(c)

-16,000 cals mol^-1

(d)

4000 cals mol^-1

When solid melts there is ____________

(a)

an increase of entropy

(b)

a decrease in entropy

(c)

an increase in free energy

(d)

an increase of heat of fusion

An efficiency of an engine is always ____________

(a)

=0%

(b)

>100%

(c)

<100%

(d)

= 100%

-\(\Delta\) G is the net work done by the system except ____________

(a)

Electrical work

(b)

Expansion work

(c)

Chemical work

(d)

Photo chemical work

Entropy change involved in the conversion of 1 mole of liquid water at 373K to vapour at the same temperature will be (\(\Delta\)H_vap=2.257 kJg^-1) ____________

(a)

0.119 kJ

(b)

0.109 kJ

(c)

0.129 kJ

(d)

0.120 kJ

Which of the following units represent largest amount of energy?

(a)

calories

(b)

Joule

(c)

erg

(d)

eV

Identify the state quantity among the following:

(a)

q

(b)

q-w

(c)

q+w

(d)

q/w

Heat liberated when 100 ml of IN NaOH is neutralized by 300 ml of IN HCI __________

(a)

22.92 kJ

(b)

17.19 kJ

(c)

11.6 kJ

(d)

5.73 kJ

In an adiabatic process, no transfer of heat takes place between the system and surroundings. Choose the convert option for free expansion of ideal gas under adiabatic conditions from the following:

(a)

q=0; \(\Delta\)T \(\neq \)0; w = 0

(b)

q\(\neq \)0;\(\Delta\)T =0; w = 0

(c)

q = 0; \(\Delta\)T = 0; w = 0

(d)

q = 0; \(\Delta\)T < 0; w \(\neq \)0

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

Which one of the following is an extensive property?

(a)

Molar volume

(b)

Density

(c)

Molarity

(d)

Entropy

Which one of the following is an intensive property??

(a)

Specific heat capacity

(b)

Mass

(c)

Enthalpy

(d)

Heat capacity

Thermodynamics is applicable to ________

(a)

macroscopic system only

(b)

microscopic system only

(c)

homogeneous system only

(d)

heterogeneous system only

Which of the following properties is not a function of state?

(a)

Concentration

(b)

Internal energy

(c)

Enthalpy

(d)

Entropy

For the process to occur under adiabatic conditions, the correct condition is __________ 

(a)

ΔT=0

(b)

Δ_P=0

(c)

q=0

(d)

w=0

The standard substance used in the enthalpy of combustion of a substance in bomb calorimeter is _______

(a)

methane

(b)

acetic acid

(c)

propane

(d)

benzoic acid

If K_b and K_f for a reversible reactions are 0.8 x 10^–5 and 1.6 x 10^–4 respectively, the value of the equilibrium constant is __________

(a)

20

(b)

0.2 x 10^-4

(c)

0.05

(d)

none of these

The formation of ammonia from N₂(g) and H₂(g) is a reversible reaction
N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + Heat
What is the effect of increase of temperature on this equilibrium reaction ______________

(a)

equilibrium is unaltered

(b)

formation of ammonia is favoured

(c)

equilibrium is shifted to the left

(d)

reaction rate does not change

Which one of the following is incorrect statement?

(a)

for a system at equilibrium, Q is always less than the equilibrium constant

(b)

equilibrium can be attained from either side of the reaction

(c)

presence of catalyst affects both the forward reaction and reverse reaction to the same extent

(d)

Equilibrium constant varied with temperature

K₁ and K₂ are the equilibrium constants for the reactions respectively.
\({ N }_{ 2 }(g)+{ O }_{ 2 }(g)\overset { { K }_{ 1 } }{ \rightleftharpoons } 2NO(g)\)
\(2NO(g)+{ O }_{ 2 }(g)\overset { { K }_{ 2 } }{ \rightleftharpoons } { 2NO }_{ 2 }(g)\)
What is the equilibrium constant for the reaction NO₂(g) ⇌ ½N₂(g) + O₂(g)

(a)

\({1\over \sqrt{K_1K_2}}\)

(b)

(K₁ = K₂)^1/2

(c)

\({1\over 2K_1K_2}\)

(d)

\(({1\over K_1K_2})^{3/2}\)

In the equilibrium,
2A(g) ⇌ 2B(g) + C₂(g)
the equilibrium concentrations of A, B and C₂ at 400 K are 1\(\times\)10^–4 M, 2.0 \(\times\)10^–3 M, 1.5 \(\times\)10^–4 M respectively. The value of K_C for the equilibrium at 400 K is ________

(a)

0.06

(b)

0.09

(c)

0.62

(d)

3 x 10^-2

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

(a)

\({1\over RT}\)

(b)

\(\sqrt{RT}\)

(c)

RT

(d)

(RT)²

For the reaction AB (g) ⇌ A(g) + B(g), at equilibrium, AB is 20% dissociated at a total pressure of P, The equilibrium constant K_P is related to the total pressure by the expression __________

(a)

P = 24 K_P

(b)

P = 8 K_P

(c)

24 P = K_P

(d)

none of these

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 ___________

(a)

0.5 - x

(b)

x + 0.5

(c)

2x + 0.5

(d)

x + 1

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 __________

(a)

36 : 1

(b)

1 : 1

(c)

3 : 1

(d)

1 : 9

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

(a)

not changed

(b)

also decreased by ¼ times

(c)

increase by 4 times

(d)

increase by 64 times

Consider the reaction where K_P = 0.5 at a particular temperature
PCl₅(g) ⇌ PCl₃ (g) + Cl₂ (g)
if the three gases are mixed in a container so that the partial pressure of each gas is initially 1 atm, then which one of the following is true ____________

(a)

more PCl₃ will be produced

(b)

more Cl₂ will be produced

(c)

more PCl₅ will be produced

(d)

none of these

In a chemical equilibrium, the rate constant for the forward reaction is 2.5 \(\times\)10² and the equilibrium constant is 50. The rate constant for the reverse reaction is ____________

(a)

11.5

(b)

5

(c)

2 x 10²

(d)

2 x 10^-3

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)

\({K_1\over 2}\)

Consider the following reversible reaction at equilibrium, A + B ⇌ C, If the concentration of the reactants A and B are doubled, then the equilibrium constant will ___________

(a)

be doubled

(b)

become one fourth

(c)

be halved

(d)

remain the same

The equilibrium constants of the following reactions are:

N2 + 3H2 ⇌ 2NH3   :	K1
N2 + O2 ⇌ 2NO      :	K2
H2 + ½O2 ⇌ H2O   :	K3

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

(a)

\(K_2^3{K_3\over K_1}\)

(b)

\(K_1{K_3^3\over K_2}\)

(c)

\(K_2{K_3^3\over K_1}\)

(d)

\(K_2{K_3\over K_1}\)