Dihydrogen gas is obtained from natural gas by partial oxidation with steam as per following endothermic reaction:

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

(a) Write as expression for $K_{p}$ for the above reaction.

(b) How will the values of $K_{p}$ and composition of equilibrium mixture be affected by
(i) increasing the pressure,
(ii) Increasing the temperature and
(iii) Using a catalyst?

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Solution

(a) The equilibrium constant expression is $K_{p} = \frac{P_{C O} \times P_{H_{2}}^{3}}{P_{C H_{4}} P_{H_{2} O}}$ .

(b) (i) As the pressure increases, the equilibrium will shift to left so that less number of moles are produced.

This is according to Le-Chatelier's principle (Refer image)

(ii) For exothermic reaction, with increase in temperature, the equilibrium will shift in the backward direction.

(iii) When a catalyst is used, the equilibrium is not disturbed. The equilibrium is quickly attained.

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Similar questions

Dihydrogen gas is obtained from natural gas by partial oxidation with steam as per following endothermic reaction:

(a) Write as expression for K_p for the above reaction.

(b) How will the values of K_p and composition of equilibrium mixture be affected by

(i) Increasing the pressure

(ii) Increasing the temperature

(iii) Using a catalyst?

Dihydrogen gas is obtained from natural gas by partial oxidation with steam as per following endothermic reaction:
(i) $C H_{4} (g) + H_{2} O (g) \leftrightarrow C O (g) + 3 H_{2} (g)$
Write as expression for $K_{p}$ for the above reaction

(ii) $C H_{4} (g) + H_{2} O (g) \leftrightarrow C O (g) + 3 H_{2} (g)$
How will the values of $K_{p}$ and compositioon of equilibrium mixture be affected by
(i) Increasing the pressure
(ii) Increasing the temperature
(iii) Using a catalyst?

Q. Methane gas and steam in equimolar amounts are taken in a flask and sealed where the following equilibrium was established:

C H_{4} (g) + H_{2} O (v) ⇌ C O (g) + 3 H_{2} (g)

2 H_{2} (g) + C O (g) ⇌ C H_{3} O H (g); K_{p} = \frac{2}{7} a t m^{- 2}

At equilibrium if partial pressure of CO(g) as found to be 0.5 atm and totaI pressure inside the flask was 5 atm. then

K_{p}

of the first reaction is: (approximately)

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 CO and H₂. In second stage, CO formed in first stage is reacted with more steam in water gas shift reaction,

If a reaction vessel at 400°C is charged with an equimolar mixture of CO and steam such that 4.0 bar, what will be the partial pressure of H₂ at equilibrium? Kp= 10.1 at 400°C