The equilibrium constant for the following reaction at 1395 K . 2 H 2 O ⇌ 2 H 2 + O 2 K 1 = 2 . 1 × 10 - 13 2 CO 2 ⇌ 2 CO + O 2 K 2 = 1 . 4 × 10 - 12 Calculate the value of K for the reaction : H 2 + CO 2 ⇌ CO + H 2 O

Equilibrium Constant - It is the ratio of concentration of products and reactants each raise to its stoichiometric constant. 2 H 2 O ⇋ 2 H 2 g + O 2 K 1 = 2 . 1 × 10 - 13 Reverse this reaction 2 H 2 g + O 2 g ⇌ 2 H 2 O K ' = 1 K 1 . . . . . . . 1 2 CO 2 g ⇋ 2 CO + O 2 K 2 = 1 . 4 × 10 - 12 . . . . . . 2 Add equation 1 and 2 2 H 2 + 2 CO 2 ⇌ 2 CO + 2 H 2 O K 3 = 1 K 1 × K 2 . . . . . 3 Divide equation 3 by 2 H 2 + CO 2 ⇋ CO + H 2 O K 3 = K 2 K 1 K 3 = 1 . 4 × 10 - 12 2 . 1 × 10 - 13 = 2 . 58

For the reaction SO 2 g + 1 2 O 2 g ⇌ SO 3 g ΔH 298 ° = - 98 . 32 kJ mole ΔS 298 ° = - 95 . 0 JK - 1 mole - 1 . Find the K p for this reaction at 298 K .

Given: ΔH 298 ° = - 98 . 32 kJ mole - 1 , ΔS 298 ° = - 95 . 0 JK - 1 mole - 1 SO 2 g + 1 2 O 2 g ⇌ SO 3 g Gibbs free energy Δ G 0 = Δ H 0 - T Δ S 0 . . . . . . . . . . . . ( 1 ) Also Δ G 0 = - R T ln K P . . . . . . . . . . ( 2 ) Where ∆ G 0 = Standard Gibbs free energy ∆ H 0 = Change in standard enthalpy ∆ S 0 = Change in standard entropy R = Gas constant By equation ( 1 ) and ( 2 ) Δ H 0 - T Δ S 0 = - R T ln K P ⇒ - 98 . 32 × 10 3 - 298 × ( - 95 ) = - 8 . 314 × 298 × ln K p ⇒ K p = 1 . 862 × 10 12 atm - 1 2

EASY

JEE Main/Advance

IMPORTANT

Earn 100

The density of an equilibrium mixture of $N_{2} O_{4}$ and ${NO}_{2}$ at $101.32 {KP}_{a}$ is $3.62 {gdm}^{- 3}$ at $288 K$ and $1.84 {gdm}^{- 3}$ at $348 K$ . What is the heat of the reaction for $N_{2} O_{4} ⇌ 2 {NO}_{2} (g)$ .

Important Questions on Equilibrium

EASY

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>EXERCISE-4>Q 10

The equilibrium constant for the following reaction at $1395 K$ .

$2 H_{2} O ⇌ 2 H_{2} + O_{2} K_{1} = 2.1 \times 10^{- 13}$

$\begin{array}{l} 2 {CO}_{2} ⇌ 2 CO + O_{2} & K_{2} = 1.4 \times 10^{- 12} \end{array}$

Calculate the value of $K$ for the reaction : $H_{2} + {CO}_{2} ⇌ CO + H_{2} O$

HARD

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>EXERCISE-4>Q 11

A saturated solution of iodine in water contains

0.33 {gI}_{2} L^{- 1}

. More than this can dissolve in a

KI

solution because of the equilibrium :

I_{2} (aq) + I^{-} (aq) ⇌ I_{3}^{-} (aq)

. A

0.10 MKI

solution

(0.10 {MI}^{-})

actually dissolves

12.5 g

of iodine

/ L

, most of which is converted to

I_{3}^{-}

. Assuming that the concentration of

I_{2}

in all saturated solutions is the same, calculate the equilibrium constant for the above reaction. What is the effect of adding water to a clear saturated of

I_{2}

in the

KI

solution?

HARD

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>EXERCISE-4>Q 12

A mixture of

N_{2}

H_{2}

are in equilibrium at

600 K

at a total pressure of

80 atm

. If the initial ratio of

N_{2}

and

H_{2}

are

3 : 1

and at equilibrium

{NH}_{3}

10 %

by volume, calculate

K_{p}

of reaction at given temperature.

HARD

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>EXERCISE-4>Q 13

$ΔG ° (298 K)$ for the reaction $\frac{1}{2 N_{2}} + 3 H_{2} ⇌ K_{1} {NH}_{3}$ is $- 16.5 kJ {mol}^{- 1}$ . Find the equilibrium constant $(K_{1})$ at $25 ° C$ . What will be the equilibrium constants $K_{2}$ and $K_{3}$ for the following reactions:

$N_{2} + 3 H_{2} ⇌ K_{2} ⇌ 2 {NH}_{3}$

${NH}_{3} ⇌ K_{3} ⇌ \frac{1}{2 N_{2}} + \frac{3}{2 H_{2}}$

HARD

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>EXERCISE-4>Q 14

For the reaction

{SO}_{2} (g) + \frac{1}{2 O_{2}} (g) ⇌ {SO}_{3} (g) {ΔH}_{298} ° = \frac{- 98.32 kJ}{mole}

{ΔS}_{298} ° = - 95.0 {JK}^{- 1} {mole}^{- 1}

. Find the

K_{p}

for this reaction at

298 K

HARD

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>EXERCISE-4>Q 15

For the reaction

C_{2} H_{6} (g) ⇌ C_{2} H_{4} (g) + H_{2} (g)

{K_{p}}^{0}

0.05

and

Δ_{r} G °

22.384 kJ {mol}^{- 1}

900 K

. If an initial mixture comprising

20 mol

C_{2} H_{6}

and

80 mol

N_{2}

(inert) is passed over a dehydrogenation catalyst at

900 K

, what is the equilibrium percentage composition of the effluent gas mixture? The total pressure is kept at

0.5

bar. Given :

Δ_{r} S ° = 135.143 J K^{- 1} {mol}^{- 1}

300 K

. Calculate

Δ_{r} G °

300 K

. (Assume

Δ_{r} C_{p} = 0)

HARD

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>EXERCISE-4>Q 16

Equimolar mixture of two gases $A_{2}$ and $B_{2}$ is taken in a container of volume $V'$ at temperature $300 K$ . At constant temperature the gases reacts according to given equations :

$A_{2} (g) ⇌ 2 A (g) k_{p} = ?$

$B_{2} (g) ⇌ 2 B (g) K_{p} = ?$

$A_{2} (g) + B_{2} (g) ⇌ 2 AB (g) k_{p} = 2$

If the initial pressure in the container was $2 atm$ and final and final pressure developed at equilibrium is $2.75$ atm in which equilibrium partial pressure of gas $AB$ was $0.5 atm$ , find equilibrium constant $k_{p}$ for the reaction.

$AB ⇌ A (g) + B (g)$

MEDIUM

JEE Main/Advance

IMPORTANT

Beta Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>EXERCISE-4>Q 17

A handbook states that the solubility of methylamine ${CH}_{3} {NH}_{2} (g)$ in water at $1 atm$ pressure at $25 ° C$ is $959$ volumes of ${CH}_{3} {NH}_{2} (g)$ per volume of water $({pk}_{b} = 3.39)$ :

(a) Estimate the max. $pH$ that can be attained by dissolving methylamine in water.

(b) What molarity $NaOH (aq .)$ would be required to yield the same $pH$ ?

The density of an equilibrium mixture of N2O4 and NO2 at 101.32 KPa is 3.62 gdm-3 at 288 K and 1.84 gdm-3 at 348 K. What is the heat of the reaction for N2O4⇌2NO2(g).

Important Questions on Equilibrium

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The density of an equilibrium mixture of $N_{2} O_{4}$ and ${NO}_{2}$ at $101.32 {KP}_{a}$ is $3.62 {gdm}^{- 3}$ at $288 K$ and $1.84 {gdm}^{- 3}$ at $348 K$ . What is the heat of the reaction for $N_{2} O_{4} ⇌ 2 {NO}_{2} (g)$ .