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For the reaction \( 2 \mathrm{H}_{2}+2 \mathrm{NO} \longrightarrow \mathrm{N}_{2}+2 \mathrm{H}_{2} \mathrm{O} \), the following mechanism has been suggested: \( 2 \mathrm{NO} \rightleftharpoons \mathrm{N}_{2} \mathrm{O}_{2} \) equilibrium constant \( \mathrm{K}_{1} \) (fast)
\( P \)
\[
\mathrm{N}_{2} \mathrm{O}_{2}+\mathrm{H}_{2} \stackrel{\mathrm{k}_{2}}{\longrightarrow} \mathrm{N}_{2} \mathrm{O}+\mathrm{H}_{2} \mathrm{O} \text { (slow) }
\]
W
\[
\mathrm{N}_{2} \mathrm{O}+\mathrm{H}_{2} \stackrel{\mathrm{k}_{3}}{\longrightarrow} \mathrm{N}_{2}+\mathrm{H}_{2} \mathrm{O} \text { (fast) }
\]
Establish the rate law for given reaction.
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