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 H_2`. In second stage, CO formed in first stage is reacted with more steam in water gas shift reaction,
` CO(g) +H_2O(g) hArr CO_2(g) + H_2(g)`
If a reaction wissel at 400°C is charged with an equimolar mixture of CO and steam such that `rho_(CO) = rho_(H_2O) 4.0` bar, what will be the partial pressure of `H_2 `at equilibrium? `K_p = 0.1` at 400° C.

Explanation

To solve the problem, we will follow these steps:

### Step 1: Write the balanced chemical equation
The balanced equation for the water gas shift reaction is:
\[ \text{CO(g)} + \text{H}_2\text{O(g)} \rightleftharpoons \text{CO}_2\text{(g)} + \text{H}_2\text{(g)} \]

### Step 2: Define initial conditions
According to the problem, we have an equimolar mixture of CO and steam, both at a partial pressure of 4 bar:
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