$$2NO + 2H_2 \rightarrow N_2 + 2H_2O$$. The above reaction has been studied at $$800°C$$.The related data are given in the table below

The order of the reaction with respect to NO is ______.

The given reaction is:

$$2NO + 2H_2 \rightarrow N_2 + 2H_2O$$

This reaction has been studied at 800°C, and the mechanism is well-established. In the first, slow, rate-determining step the following occurs: $$2NO + H_2 \rightarrow N_2O + H_2O$$. A fast second step then follows: $$N_2O + H_2 \rightarrow N_2 + H_2O$$.

Since the first step is rate-determining, the rate law is determined by this step, giving: $$\text{Rate} = k[NO]^2[H_2]$$.

From the rate law, the order with respect to NO is the exponent of [NO], which is 2. Therefore, the order of the reaction with respect to NO is $$\textbf{2}$$.