In which one of the following equilibria, K p ≠ K c ?

N O 2 g + S O 2 g ⇌ N O g + S O 3 g

For the reaction: 2 NO 2 g ⇌ 2 NO g + O 2 g , K c = 1 .8 × 10 - 6 at 184 o C , R = 0 .0831 J / molK When K p and K c are compared at 184 o C. It is found that

Whether K p is greater than, less than or equal to K c depends upon the total gas pressure.

MEDIUM

Earn 100

Derive the equilibrium constant in terms of mole fraction for a given reaction.

$aA ⇌ bB$

Important Questions on Equilibria

EASY

Chemistry>Physical Chemistry>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

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)

HARD

Chemistry>Physical Chemistry>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

Consider the equilibrium

X_{2} + Y_{2} ⇌ P

. Find the stoichiometric coefficient of the

P

using the data given in the following table:

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

MEDIUM

Chemistry>Physical Chemistry>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

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:

MEDIUM

Chemistry>Physical Chemistry>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

For the following reaction, equilibrium constant are given:

$S (s) + O_{2} (g) ⇌ S O_{2} (g); K_{1} = 10^{52}$

$2 S (s) + 3 O_{2} (g) ⇌ 2 S O_{3} (g); K_{2} = 10^{129}$

The equilibrium constant for the reaction, $2 {S O}_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)$ is:

EASY

Chemistry>Physical Chemistry>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

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:

EASY

Chemistry>Physical Chemistry>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

A solid $XY$ kept in an evacuated sealed container undergoes decomposition to form a mixture of gases $X and Y$ at temperature $T$ .

The equilibrium pressure is $10 bar$ in this vessel. $K_{p}$ for this reaction is?

HARD

Chemistry>Physical Chemistry>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

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)

EASY

Chemistry>Physical Chemistry>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

The value of $K_{c}$ for the reaction:

$A + 3 B ⇌ 2 C at 400 ° C$ is $0.5 mol L^{- 1} .$ Calculate the value of $K_{P}$ in $atm$ .

HARD

Chemistry>Physical Chemistry>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

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>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

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>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

In which one of the following equilibria,

K_{p} \neq K_{c} ?

MEDIUM

Chemistry>Physical Chemistry>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

For the reaction:

2 {NO}_{2 (g)} ⇌ 2 {NO}_{(g)} + O_{2 (g)},

(K_{c} = 1 .8 \times 10^{- 6} at 184^{o} C), (R = 0 .0831 J / molK)

When

K_{p}

and

K_{c}

are compared at

184^{o} C.

It is found that

MEDIUM

Chemistry>Physical Chemistry>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

In the figure shown below reactant

A

(represented by square) is in equilibrium with product

B

(represented by circle). The equilibrium constant is (approx):

Question Image

MEDIUM

Chemistry>Physical Chemistry>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

At a certain temperature, only 50% HI is dissociated into H₂ and I₂ at equilibrium. The equilibrium constant is :

EASY

Chemistry>Physical Chemistry>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

If the equilibrium constant for

A ⇌ B + C

K_{eq}^{(1)}

and that of

B + C ⇌ P

K_{eq}^{(2)},

the equilibrium constant for

A ⇌ P

is :

EASY

Chemistry>Physical Chemistry>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

For the given equilibrium reaction,

2 A (g) ⇌ 2 B (g) + C (g)

the equilibrium constant

(K_{c})

1000 K

4 \times 10^{- 4}

. Calculate

K_{p}

for the reaction at

800 K

temperature

EASY

Chemistry>Physical Chemistry>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

4

moles of

A

are mixed with

4

moles of

B

. At equilibrium for the reaction

A + B ⇌ C + D, 2

moles of

C

and

D

are formed, the equilibrium constant for the reaction will be,

EASY

Chemistry>Physical Chemistry>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

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:

HARD

Chemistry>Physical Chemistry>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

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}

HARD

Chemistry>Physical Chemistry>Equilibria>Law of Chemical Equilibrium and Equilibrium Constants

Given that the equilibrium constant for the reaction

2 S O_{2 (g)} + O_{2 (g)} ⇌ 2 S O_{3 (g)}

has a value of 278 at a particular temperature. What is the value of the equilibrium constant for the following reaction at the same temperature?

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

Derive the equilibrium constant in terms of mole fraction for a given reaction. aA ⇌ bB

Important Questions on Equilibria

Learn and Prepare for any exam you want !

Derive the equilibrium constant in terms of mole fraction for a given reaction.

$aA ⇌ bB$