Consider the following reaction,
\( 2\text{H}_2(\text{g}) + 2\text{NO}(\text{g}) \rightarrow \text{N}_2(\text{g}) + 2\text{H}_2\text{O}(\text{g}) \)
which follows the mechanism given below:
$2\text{NO(g)} \overset{k_1}{\underset{k_{-1}}{\rightleftharpoons}} \text{N}_2\text{O}_2\text{(g)} \qquad \text{(fast equilibrium)}$
\( \text{N}_2\text{O}_2(\text{g}) + \text{H}_2(\text{g}) \xrightarrow{k_{2}} \text{N}_2\text{O}(\text{g}) + \text{H}_2\text{O}(\text{g}) \) (slow reaction)
\( \text{N}_2\text{O}(\text{g}) + \text{H}_2(\text{g}) \xrightarrow{k_{3}} \text{N}_2(\text{g}) + \text{H}_2\text{O}(\text{g}) \) (fast reaction)
The order of the reaction is ______.
