AP Chemistry
5.9 Pre-Equilibrium Approximation
5.8 Reaction Mechanism and Rate Law
The oxidation of nitric oxide to nitrogen dioxide is represented by the overall balanced equation below.
\[ 2\,\text{NO}(g) + \text{O}_2(g) \rightarrow 2\,\text{NO}_2(g) \]
A proposed two-step mechanism for the reaction consists of a fast reversible first step followed by a slow second step:
\[ \text{Step 1: } 2\,\text{NO}(g) \underset{k_{-1}}{\overset{k_1}{\rightleftharpoons}} \text{N}_2\text{O}_2(g) \quad (\text{fast pre-equilibrium}) \]
\[ \text{Step 2: } \text{N}_2\text{O}_2(g) + \text{O}_2(g) \xrightarrow{k_2} 2\,\text{NO}_2(g) \quad (\text{slow}) \]
Which of the following rate law expressions is consistent with this proposed mechanism?
\[ 2\,\text{NO}(g) + \text{O}_2(g) \rightarrow 2\,\text{NO}_2(g) \]
A proposed two-step mechanism for the reaction consists of a fast reversible first step followed by a slow second step:
\[ \text{Step 1: } 2\,\text{NO}(g) \underset{k_{-1}}{\overset{k_1}{\rightleftharpoons}} \text{N}_2\text{O}_2(g) \quad (\text{fast pre-equilibrium}) \]
\[ \text{Step 2: } \text{N}_2\text{O}_2(g) + \text{O}_2(g) \xrightarrow{k_2} 2\,\text{NO}_2(g) \quad (\text{slow}) \]
Which of the following rate law expressions is consistent with this proposed mechanism?
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