Consider the following gaseous equilibrium reactions (I), (II) and (III) with equilibrium constants \(\mathrm{K}_1, \mathrm{~K}_2\) and \(\mathrm{K}_3\) respectively
I) \(\frac{1}{2} \mathrm{~N}_2+\frac{3}{2} \mathrm{H}_2 \rightleftharpoons \mathrm{NH}_3\)
II) \(2 \mathrm{NO} \rightleftharpoons \mathrm{N}_2+\mathrm{O}_2\)
III) \(\mathrm{H}_2+\frac{1}{2} \mathrm{O}_2 \rightleftharpoons \mathrm{H}_2 \mathrm{O}\)
The correct expression for the equilibrium constant for the gaseous equilibrium reaction \(2 \mathrm{NH}_3+\frac{5}{2} \mathrm{O}_2 \rightleftharpoons 2 \mathrm{NO}+3 \mathrm{H}_2 \mathrm{O}\) is

1. A \(\frac{\mathrm{K}_3^2}{\mathrm{~K}_1 \times \mathrm{K}_2}\)
2. B \(\frac{\mathrm{K}_3^3}{\mathrm{~K}_1^2 \times \mathrm{K}_2}\)
3. C \(\frac{\mathrm{K}_3^2}{\mathrm{~K}_1^2 \times \mathrm{K}_2}\)
4. D \(\frac{\mathrm{K}_3}{\mathrm{~K}_1^{1 / 2} \times \mathrm{K}_2^2}\)