Chemical EquilibriumHard

Question

The equilibrium constant for the reaction N2(g) + O2(g) $\rightleftharpoons$2NO(g) is 0.09 at 3500 K. The fraction of equimolar mixture of N2 and O2 converted into NO is

Options

A.0.13
B.0.23
C.0.30
D.0.357

Solution

N2 + O2 $\rightleftharpoons$ 2NO

Equilibrium moles 1 – x 1 – x 2x

$0.09 = \frac{(2x)^{2}}{(1 - x)(1 - x)} \Rightarrow x = 0.13$

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