The equilibrium constant ( K p ) for the decomposition of gaseous H 2 O H 2 O g ⇌ H 2 g + 1 2 O 2 ( g ) is related to degree of dissociation ( α ) at a total pressure p is given by

K p = α 3 / 2 p 1 / 2 1 - α 2 + α 1 / 2

K p = α 3 p 1 / 2 1 + α 2 + α 1 / 2

K p = α 3 p 3 / 2 1 - α 2 + α 1 / 2

K p = α 3 / 2 p 2 1 - α 2 + α 1 / 2

EASY

Earn 100

Apply the law of mass action to the following equilibria: Formation of ${SO}_{3}$ from ${SO}_{2}$ and $O_{2}$ .

Important Questions on Equilibrium

EASY

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

For

{NH}_{4} HS (s) ⇌ {NH}_{3} (g) + H_{2} S (g)

the
observed pressure for the reaction mixture in equilibrium is

1.12 atm

106 ° C

. What is the value of

K_{p}

for the reaction?

HARD

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

4.0

moles of argon and

5.0

moles of

{PCl}_{5}

are introduced into an evacuated flask of

100

litre capacity at

610 K

. The system is allowed to equilibrate. At equilibrium, the total pressure of mixture was found to be

6.0 atm

. The

K_{p}

for the reaction is [Given :

R = 0.082 L

atm

K^{- 1} {mol}^{- 1}

]

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

A homogeneous ideal gaseous reaction

{AB}_{2 (g)} ⇌ A_{(g)} + 2 B_{(g)}

is carried out in a

25 litre

flask at

27 ° C

. The initial amount of

{AB}_{2}

was

1

mole and the equilibrium pressure was

1.9 atm

. The value of

K_{p}

x \times 10^{- 2}

. The value of

x

is (Integer answer)

[R = 0.08206 {dm}^{3} atm K^{- 1} {mol}^{- 1}]

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

For the reaction

$H_{2 (g)} + {CO}_{2 (g)} ⇌ {CO}_{(g)} + H_{2} O_{(g)},$ if the initial concentration of $[H_{2}] = [{CO}_{2}] = 1 M$ and $x$ moles $/ L$ of $H_{2}$ is consumed at equilibrium, the correct expression of $K_{P}$ is.

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

60 ° C

, dinitrogen tetroxide is fifty percent dissociated. Find its standard free energy change at this temperature and one atmosphere. [ Given:

\log 1.33 = 0.1239

]

HARD

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

For the reaction

A_{(g)} ⇌ B_{(g)} + C_{(g)}, A

33 %

dissociated at a total pressure

P .

The correct relation between

P

and

K_{p}

HARD

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

For a reaction at equilibrium

$A (g) ⇌ B (g) + \frac{1}{2} C (g)$

the relation between dissociation constant $(K)$ , degree of dissociation $(α)$ and equilibrium pressure $(p)$ is given by :

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

A sample of

HI (g)

is placed in a flask at a pressure of

0.2 atm .

At equilibrium, partial pressure of

HI (g)

0.04 atm .

What is

Kp

for the given equilibrium ?

2 HI (g) ⇌ H_{2} (g) + I_{2} (g)

HARD

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

20 litre

container at

400 K

contains

{CO}_{2} (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 the pressure of

{CO}_{2}

attains its maximum value, will be:

(Given that : {SrCO}_{3} (s) ⇌ SrO (s) + {CO}_{2} (g), K_{p} = 1 .6 atm)

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

In a closed system :

A (s) \underset{}{⇌} 2 B (g) + 3 C(g)

, if the partial pressure of C is doubled, then partial pressure of

B

will be

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

The equilibrium constant

(K_{p})

for the decomposition of gaseous

H_{2} O

H_{2} O (g) ⇌ H_{2} (g) + \frac{1}{2} O_{2} (g)

is related to degree of dissociation

(α)

at a total pressure

p

is given by

HARD

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

For the equilibrium

{N H}_{4} H S (s) ⇌ {N H}_{3} (g) + H_{2} S (g)

K_{c} = 1.8 \times 10^{- 4}

298 K

. The value of

K_{p}

298 K

would be -

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

The decomposition reaction,

4 {H N O}_{3} (g) ⇄ 4 {N O}_{2} (g) + 2 H_{2} O (g) + O 2 (g)

is started with pure

{H N O}_{3} (g)

. If p is the total pressure at equilibrium, then

EASY

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

For the reaction,

H_{2} (g) + I_{2} (g) ⇌ 2 H I (g)

, the equilibrium constants expressed in terms of concentration

K_{c}

and in terms of partial pressure

K_{p}

, are related to each other as:

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

${N H}_{4} {C O O N H}_{2} (s) ⇌ 2 {N H}_{3} (g) + {C O}_{2} (g)$

If equilibrium pressure is $3 a t m$ for the above reaction; $K_{p}$ will be:

HARD

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

Dihydrogen gas used in Haber’s process is produced by reacting methane from natural gas with high-temperature steam. The first stage of two stage reaction involves the formation of

C O

and

H_{2}

. In second stage,

C O

formed in first stage is reacted with more steam in water gas shift reaction,

C O (g) + H_{2} O (g) ⇌ C O_{2} (g) + H_{2} (g)

If a reaction vessel at

400^{o} C

is charged with an equimolar mixture of

C O

and steam such that

p_{CO} = p_{H_{2} O} = 4.0

bar, what will be the partial pressure of

H_{2}

at equilibrium?

K_{p} = 10.1 a t 400 ° C

HARD

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

For the reaction,

2 H I (g) ⇌ H_{2} (g) + I_{2} (g)

the degree of dissociation

(α)

H I (g)

is related to equilibrium constant

K_{p}

by the expression

HARD

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

0.2 mole of

N H_{4} C l

are introduced into an empty container of 10 litre and heated to

327^{o} C

to attain equilibrium as :

N H_{4} C l_{(s)} \to N H_{3 (g)} + H C l_{(g)}; (K_{P} = 0.36 a t m^{2})

The quantity of solid

N H_{4} C l

left is:

HARD

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

At same temperature N₂O₄ is dissociated to 40% and 50% at total pressure p₁ and p₂ atm respectively in NO₂. Then the ratio of p₁ and p₂ is

EASY

Chemistry>Physical Chemistry>Equilibrium>Homogeneous Equilibria

A vessel at

1000 K

contains

C O_{2}

with a pressure of

0.5 atm

. Some of the

C O_{2}

is converted into

CO

on the addition of graphite. If the total pressure at equilibrium is

0.8 atm

, then the value of

K_{p}

is:

Apply the law of mass action to the following equilibria: Formation of SO3 from SO2 and O2.

Important Questions on Equilibrium

Learn and Prepare for any exam you want !

Apply the law of mass action to the following equilibria: Formation of ${SO}_{3}$ from ${SO}_{2}$ and $O_{2}$ .