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\[
\begin{array}{l}
\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g}), \mathrm{K}_{1} \\
\mathrm{~N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g}), \mathrm{K}_{2} \\
\mathrm{H}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{H}_{2} \mathrm{O}(\mathrm{g}), \mathrm{K}_{3}
\end{array}
\]
The equation for the equilibrium constant of the reaction
\( 2 \mathrm{NH}_{3}(\mathrm{~g})+\frac{5}{2} \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}),\left(K_{4}\right) \) in terms of \( \mathrm{K}_{1}, \mathrm{~K}_{2} \) and \( \mathrm{K}_{3} \) is:
(a) \( \frac{\mathrm{K}_{1} \cdot \mathrm{K}_{2}}{\mathrm{~K}_{3}} \)
(b) \( \frac{\mathrm{K}_{1} \cdot \mathrm{K}_{3}^{2}}{\mathrm{~K}_{2}} \)
(c) \( \mathrm{K}_{1} \mathrm{~K}_{2} \mathrm{~K}_{3} \)
(d) \( \frac{\mathrm{K}_{2} \cdot \mathrm{K}_{3}^{3}}{\mathrm{~K}_{1}} \)
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