If the value of an equilibrium constant for a particular reaction is 1.6 × 10 12 , then at equilibrium the system will contain:

Similar amounts of reactants and products

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At $700 K$ , the equilibrium constant $K_{p}$ for the reaction $2 S O_{3 (g)} ⇌ 2 S O_{2 (g)} + O_{2 (g)}$ is $1.80 \times 1 0^{- 3}$ ${k P}_{a}$ , ( $R = 8.314 {J k}^{- 1} {m o l}^{- 1}$ ). The numerical value in moles per litre of $K_{c}$ for this reaction at the same temperature will be

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Important Questions on Equilibrium

EASY

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

Consider the following reversible chemical reactions:

A_{2} (g) + B_{2} (g) \overset{k_{1}}{⇌} 2 A B (g)

.....(1)

6 A B (g) \overset{k_{2}}{⇌} 3 A_{2} (g) + 3 B_{2} (g)

.....(2)

The relation between

K_{1}

and

K_{2}

is:

HARD

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

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}

]

HARD

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

What are the values of

\frac{K_{p}}{K_{c}}

for the following reactions at

300 K

respectively?

(At

300 K, RT = 24 .62 {dm}^{3} atm {mol}^{- 1}

)

N_{2} (g) + O_{2} (g) ⇌ 2 NO (g); \frac{K_{p}}{K_{c}} = x_{1}

N_{2} O_{4} (g) ⇌ 2 {NO}_{2} (g); \frac{K_{p}}{K_{c}} = x_{2}

N_{2} (g) + 3 H_{2} (g) ⇌ 2 {NH}_{3} (g); \frac{K_{p}}{K_{c}} = x_{3}

EASY

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

If the value of an equilibrium constant for a particular reaction is

1.6 \times 10^{12}

, then at equilibrium the system will contain:

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

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

]

EASY

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

If the equilibrium constant for

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

is K, the equilibrium constant for

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

will be:

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

In a chemical reaction,

A + 2 B \overset{K}{⇌} 2 C + D

, the initial concentration of

B

was

1.5

times of the concentration of

A

, but the equilibrium concentrations of

A

and

B

were found to be equal. The equilibrium constant

(K)

for the chemical reaction is:

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

Consider the equilibria

(i) a n d (i i)

with equilibrium constants

K_{1} a n d K_{2}

, respectively

{SO}_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ {SO}_{3} (g)

.... (i)

2 {SO}_{3} (g) ⇌ 2 {SO}_{2} (g) + O_{2} (g)

.... (ii)

K_{1} a n d K_{2}

are related as

HARD

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

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}

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

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.

HARD

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

Consider the equilibrium

X_{2} + Y_{2} ⇌ P

. Find the stoichiometric coefficient of the

P

using the data given in the following table:

$X_{2} / m o l L^{- 1}$	$Y_{2} / m o l L^{- 1}$	$P / m o l L^{- 1}$
$1.14 \times 10^{- 2}$	$0.12 \times 10^{- 2}$	$2.52 \times 10^{- 2}$
$0.92 \times 10^{- 2}$	$0.22 \times 10^{- 2}$	$3.08 \times 10^{- 2}$

EASY

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

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?

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

For the reaction,

A ⇌ n B

the concentration of A decreases from

0.06 t o 0.03 m o l L^{- 1}

and that of B rises from

0 t o 0.06 m o l L^{- 1}

at equilibrium. The values of n and the equilibrium constant for the reaction, respectively, are

HARD

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

5 .1 g {NH}_{4} SH

is introduced in

3 .0 L

evacuated flask at

327^{o} C

30 %

of the solid

{NH}_{4} SH

is decomposed to

{NH}_{3}

and

H_{2} S

as gases. The

K_{P}

of the reaction at

327^{o} C

(R = 0 .082 L atm {mol}^{- 1} K^{- 1}, Molar mass of S = 32 g {mol}^{- 1}, Molar mass of N = 14 g {mol}^{- 1})

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

The equilibrium constants of the following are:

\begin{matrix} N_{2} + 3 H_{2} ⇌ 2 {NH}_{3} & K_{1} \\ N_{2} + O_{2} ⇌ 2 NO & K_{2} \\ H_{2} + \frac{1}{2} O_{2} \to H_{2} O & K_{3} \end{matrix}

The equilibrium constant (

K

) of the reaction:

2 N H_{3} + \frac{5}{2} O_{2} \overset{K}{⇌} 2 N O + 3 H_{2} O

, will be:

EASY

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

For the reaction

{SO}_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ {SO}_{3} (g)

, if

K_{P} = K_{C} {(RT)}^{x}

where the symbols have usual meaning then the value of

x

is:
(assuming ideality)

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

The equilibrium constant

(K_{c})

of two reactions

H_{2} + I_{2} ⇌ 2 HI and N_{2} + 3 H_{2} ⇌ 2 {NH}_{3}

are

50 and 1000

, respectively. The equilibrium constant of the reaction

N_{2} + 6 HI ⇌ 2 {NH}_{3} + 3 I_{2}

is closest to:

HARD

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

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>Equilibrium Constants and its Significance

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>Equilibrium Constants and its Significance

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)

At 700 K, the equilibrium constant Kp for the reaction 2SO3(g)⇌2SO2(g)+O2(g) is 1.80×10-3 kPa, (R=8.314 Jk-1 mol–1). The numerical value in moles per litre of Kc for this reaction at the same temperature will be

Important Questions on Equilibrium

Learn and Prepare for any exam you want !

At $700 K$ , the equilibrium constant $K_{p}$ for the reaction $2 S O_{3 (g)} ⇌ 2 S O_{2 (g)} + O_{2 (g)}$ is $1.80 \times 1 0^{- 3}$ ${k P}_{a}$ , ( $R = 8.314 {J k}^{- 1} {m o l}^{- 1}$ ). The numerical value in moles per litre of $K_{c}$ for this reaction at the same temperature will be