Nitrogen monoxide reacts with hydrogen gas to produce...

Nitrogen monoxide reacts with hydrogen gas to produce nitrogen and water vapor. The mechanism is believed to be: Step 1: 2NO(g) → N2O2(g) (slow) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) Step 3: N2O(g) + H2(g) → N2(g) + H2O(g) Write an overall balanced equation for this process (show your work). Identify the reaction intermediates. Write the rate equation for this reaction.

Nitrogen monoxide is reduced by hydrogen to give water and nitrogen $$2 \mathrm{H}_{2}(\mathrm{~g})+2 \mathrm{NO}(\mathrm{g}) \longrightarrow \mathrm{N}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})$$ and one possible mechanism for this reaction is a sequence of three elementary steps. Step 1 (fast): $$2 \mathrm{NO}(\mathrm{g}) \rightleftharpoons \mathrm{N}_{2} \mathrm{O}_{2}(\mathrm{~g})$$ Step $2($ slow $): \mathrm{N}_{2} \mathrm{O}_{2}(\mathrm{~g})+\mathrm{H}_{2}(\mathrm{~g}) \longrightarrow \mathrm{N}_{2} \mathrm{O}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})$ Step 3 (fast): $\mathrm{N}_{2} \mathrm{O}(\mathrm{g})+\mathrm{H}_{2}(\mathrm{~g}) \longrightarrow \mathrm{N}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})$ (a) Show that the sum of these steps gives the net reaction. (b) What is the rate law for this reaction?

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