At \( 298 \, \mathrm{K} \)
\( \mathrm{N}_2(\mathrm{g}) + 3\mathrm{H}_2(\mathrm{g}) \rightleftharpoons 2\mathrm{NH}_3(\mathrm{g}), \, K_1 = 4 \times 10^{5} \)
\( \mathrm{N}_2(\mathrm{g}) + \mathrm{O}_2(\mathrm{g}) \rightleftharpoons 2\mathrm{NO}(\mathrm{g}), \, K_2 = 1.6 \times 10^{12} \)
\( \mathrm{H}_2(\mathrm{g}) + \tfrac{1}{2}\mathrm{O}_2(\mathrm{g}) \rightleftharpoons \mathrm{H}_2\mathrm{O}(\mathrm{g}), \, K_3 = 10^{-13} \)
Based on above equilibria, the equilibrium constant of the reaction,
\( 2\mathrm{NH}_3(\mathrm{g}) + \tfrac{5}{2}\mathrm{O}_2(\mathrm{g}) \rightleftharpoons 2\mathrm{NO}(\mathrm{g}) + 3\mathrm{H}_2\mathrm{O}(\mathrm{g}) \) is _______ \( \times 10^{-33} \)
