At 298 K N_2( g )+3 H_2( g ) ⇌ 2 NH_3( g ), K_1=4 × 10^5; N_2( g )+ O_2( g ) ⇌ 2 NO ( g ), K_2=1.6 × 10^12; H_2( g )+1/2 O_2( g ) ⇌ H_2 O ( g ),…

At $\displaystyle 298$ K $$\begin{aligned} & \mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g}), \mathrm{K}_1=4 \times 10^5 \\ & \mathrm{~N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{~g}), \mathrm{K}_2=1.6 \times 10^{12} \\ & \mathrm{H}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightleftharpoons \mathrm{H}_2 \mathrm{O}(\mathrm{~g}), \mathrm{K}_3=1.0 \times 10^{-13} \end{aligned} $$ Based on above equilibria, the equilibrium constant of the reaction, $\displaystyle 2 \mathrm{NH}_3(\mathrm{~g})+\frac{5}{2} \mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})+3 \mathrm{H}_2 \mathrm{O}(\mathrm{g})$ is $\displaystyle \_\_\_\_$ $\displaystyle \times 10^{-33}$ (Nearest integer).