Question

The following equilibrium constants are given:
$$\begin{aligned} &\mathrm{N}_{2}+3 \mathrm{~N}_{2} \rightleftharpoons 2 \mathrm{NH}_{3} ; \mathrm{K}_{1} \\ &\mathrm{~N}_{2}+\mathrm{O}_{2} \rightleftharpoons 2 \mathrm{NO} ; \mathrm{K}_{2} \\ &\mathrm{H}_{2}+\frac{1}{2} \mathrm{O}_{2} \rightleftharpoons \mathrm{H}_{2} \mathrm{O} ; \mathrm{K}_{3} \end{aligned}$$
The equilibrium constant for the oxidation of $2 \mathrm{~mol}$ of $\mathrm{NH}_{3}$ to give $\mathrm{NO}$ is
(A) $\mathrm{K}_{1} \cdot \frac{\mathrm{K}_{2}}{\mathrm{~K}_{3}}$
(B) $\mathrm{K}_{2} \cdot \frac{\mathrm{K}_{3}^{3}}{\mathrm{~K}_{1}}$
(C) $\mathrm{K}_{2} \cdot \frac{\mathrm{K}_{3}^{2}}{\mathrm{~K}_{1}}$
(D) $\mathrm{K}_{2}^{2} \cdot \frac{\mathrm{K}_{3}}{\mathrm{~K}_{1}}$
Ans: (B)

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