Chemical EquilibriumHard

Question

The equilibrium constant for the reaction CO(g) + H2O(g) $\rightleftharpoons$CO2(g) + H2(g) is 3.0 at 500 K. In a 2.0 L vessel, 60 g of water gas [equimolar mixture of CO(g) and H2(g)] and 90 g steam is initially taken. What is the equilibrium concentration of H2(g)?

Options

A.1.75 M
B.3.5 M
C.1.5 M
D.0.75 M

Solution

CO(g) + H2O(g) $\rightleftharpoons$ CO2(g) + H2(g)

Initial moles 2 5 0 2

Equilibrium moles 2 – x 5 – x x 2 + x

Now, $K_{eq} = 3.0 = \frac{x.(2 + x)}{(2 - x)(5 - x)} \Rightarrow x = 1.5$

$\therefore\left\lbrack H_{2} \right\rbrack = \frac{2 + x}{2} = 1.75\text{ M}$

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