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

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

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)

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

Equimolar concentrations of H₂ and I₂ are heated to equilibrium in a 1 litre flask. What percentage of initial concentration of H₂ has reacted at equilibrium if rate constant for both forward and reverse reactions are equal ____________

(a)

33%

(b)

66%

(c)

(33)²%

(d)

16.5%

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

(a)

2 litre

(b)

5 litre

(c)

10 litre

(d)

4 litre

In which of the following does the reaction go almost to completion?

(a)

K_c = 10³

(b)

K_c = 10²

(c)

K_c = 10^-2

(d)

K_c= 10^-3

XY₂ dissociates as,\(XY_{ 2\left( g \right) }\rightleftharpoons { XY }_{ \left( g \right) }+Y_{ \left( g \right) }\) Initial pressure of XY₂ is 600mm Hg. The total pressure at equilibrium is 800mm Hg. Assuming volume of system to remain constant, the value of K_p is ______________

(a)

50

(b)

100

(c)

400

(d)

20

In melting of ice, which one of the conditions will be more favorable?

(a)

high temperature and high pressure

(b)

low temperature and low pressure

(c)

low temperature and high pressure

(d)

high temperature and low pressure

A state of equilibrium is reached when _____________

(a)

The rate of forward reaction is greater than the rate of the reverse reaction

(b)

The concentration of the products and reactants are equal

(c)

More product is present than rea

(d)

The concentration of the products and reactants have reached constant value

The numerical, value of equilibrium constant depends on _____________

(a)

temperature

(b)

pressure

(c)

concentration of reactants

(d)

all of these

The favourable conditions for melting of ice is ________

(a)

Low pressure

(b)

High pressure

(c)

Low temperature

(d)

Absence of catalyst

The value of AH for the reaction
\({ X }_{ 2\left( g \right) }+4Y_{ 2\left( g \right) }\rightleftharpoons 2XY_{ 4\left( g \right) }\) is less than zero. Formation of XY_4(g) will be favoured at :

(a)

High pressure and low temperature

(b)

Low pressure and low temperature

(c)

High temperature and high pressure

(d)

High temperature and low pressure.

The value of equilibrium constant of the reaction,
\({ HI }_{ \left( g \right) }\rightleftharpoons \cfrac { 1 }{ 2 } { H }_{ 2\left( g \right) }+\cfrac { 1 }{ 2 } { I }_{ 2\left( g \right) }\) is 8.0. The equilibrium constant of the reaction; \({ H }_{ 2\left( g \right) }+I_{ 2\left( g \right) }\rightleftharpoons { 2HI }_{ \left( g \right) }\)

(a)

\(\cfrac { 1 }{ 8 } \)

(b)

\(\cfrac { 1 }{ 16 } \)

(c)

16

(d)

\(\cfrac { 1 }{ 64 } \)

In the manufacture of NH₃ by Haber's process involving the reaction.\({ N }_{ 2\left( g \right) }+{ 3H }_{ 2\left( g \right) }\overset { \left[ { Fe }_{ 2 }{ O }_{ 2 } \right] }{ \rightleftharpoons } 2{ NH }_{ 3\left( g \right) }\) \(\Delta H\)=-22.08 kcal. The favourable conditions are ___________

(a)

High pressure and low temperature

(b)

High pressure and high temperature

(c)

Low pressure and high temperature

(d)

Low pressure and low temperature

Sulphide ion reacts with solid sulphur
\({ S }_{ \left( aq \right) }^{ 2- }+{ S }_{ \left( s \right) }\rightleftharpoons { S }_{ 2\left( aq \right) }\) K₁ = 10
\({ S }_{ \left( aq \right) }^{ 2- }+{ 2S }_{ \left( s \right) }\rightleftharpoons { S }_{ 3\left( aq \right) }\) K₂ = 130 
The equilibrium constant for the formation of \({ S }_{ 3 }^{ 2- }\left( aq \right) \) and \({ S }_{ 2 }^{ 2- }\left( aq \right) \) 

(a)

10

(b)

13

(c)

130

(d)

1300

The active mass of 7.0 g of nitrogen in a 2.0 L container would be ____________

(a)

0.25

(b)

0.125

(c)

0.5

(d)

14.0

Equilibrium constant Kp for following reaction
\(MgCO_{ 3\left( s \right) }\rightleftharpoons Mg{ O }_{ \left( s \right) }+{ CO }_{ 2\left( g \right) }\)

(a)

K_p = P_co2

(b)

\({ K }_{ p }=\cfrac { { p }_{ { CO }_{ 2 } }\times { p }_{ CO_{ 2 } }\times { p }_{ Mgo } }{ { P }_{ MrCO } } \)

(c)

\({ K }_{ p }=\cfrac { { P }_{ MG }{ CO }_{ 3 } }{ { P }_{ CO\bullet }p_{ mgO } } \)

(d)

\({ K }_{ p }=\cfrac { { P }_{ MG }{ CO }_{ 3 } }{ { P }_{ CO\bullet }p_{ mgO } } \)

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

(a)

27

(b)

9

(c)

18

(d)

3

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

(a)

(mol dm^-3)^-1

(b)

(mol dm^-3)

(c)

(mol dm^-3)¹⁰

(d)

(mol dm-³)⁹

Which one of the following equation is not correct?

(a)

∆G^o = - RTlnK

(b)

∆G^o = ∆H^o -T∆S^o 

(c)

-RTlnK = ∆H^o -T∆S^o 

(d)

ln k = \(\frac { \Delta { H }^{ o } }{ T } -\frac { \Delta { S }^{ o } }{ R } \)