Reaction between \( \mathrm{NO} \) and \( \mathrm{O}_{2} \) to form \( \mathrm{NO}_{2} \) is \( ...
0Reaction between \( \mathrm{NO} \) and \( \mathrm{O}_{2} \) to form \( \mathrm{NO}_{2} \) is \( 2 \mathrm{NO}+\mathrm{O}_{2} \longrightarrow 2 \mathrm{NO}_{2} \) follows the following mechanism
\[
\begin{array}{l}
\mathrm{NO}+\mathrm{NO} \underset{\mathrm{k}-1}{\stackrel{\mathrm{k}_{1}}{\rightleftharpoons}} \mathrm{N}_{2} \mathrm{O}_{2} \quad \text { (in rapid equilibrium) } \\
\mathrm{N}_{2} \mathrm{O}_{2}+\mathrm{O}_{2} \stackrel{\mathrm{k}_{2}}{\longrightarrow} 2 \mathrm{NO}_{2} \quad \text { (slow) } \\
\end{array}
\]
\( P \)
W.
Show that the rate of reaction is given by
\[
-\frac{1}{2}\left(\frac{\mathrm{d}\left[\mathrm{NO}_{2}\right]}{\mathrm{dt}}\right)=\mathrm{K}[\mathrm{NO}]^{2}\left[\mathrm{O}_{2}\right]
\]
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