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,

$$CO(g)+H_{2}O(g) ⇌ CO_{2}(g)+H_{2}(g)$$

If a reaction vessel at 400°C is charged with an equimolar mixture of CO and steam such that Pco=PH2O= 4.0 bar, what will be the partial pressure of H2 at equilibrium? Kp= 10.1 at 400°C

Asked by Abhisek | 11 months ago |  92

Solution :-

Let the partial pressure of both carbon dioxide and hydrogen gas be p. The given reaction is:

CO(g)  + H2O  ⇌  CO2(g)  +  H2(g)

Initial conc.        4.0 bar          4.0 bar     0      0

At equilibrium      4.0-p           4.0-p       p       p

Given Kp = 10.1

So, partial pressure of His 3.04 bar at equilibrium.

Answered by Pragya Singh | 11 months ago

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