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)
