AP Chemistry
5.9 Pre-Equilibrium Approximation
5.8 Reaction Mechanism and Rate Law
The reaction between \(\text{NO}(g)\) and \(\text{Cl}_2(g)\) is represented by the following equation:
\[ 2\text{NO}(g) + \text{Cl}_2(g) \rightarrow 2\text{NOCl}(g) \]
A chemist proposes the following two-step mechanism for the reaction:
\[ \text{Step 1 (fast equilibrium):}\quad \text{NO}(g) + \text{Cl}_2(g) \underset{k_{-1}}{\overset{k_1}{\rightleftharpoons}} \text{NOCl}_2(g) \]
\[ \text{Step 2 (slow):}\quad \text{NOCl}_2(g) + \text{NO}(g) \xrightarrow{k_2} 2\text{NOCl}(g) \]
Based on this mechanism, which of the following is the correct rate law expression for the overall reaction in terms of elementary rate constants and reactant concentrations?
\[ 2\text{NO}(g) + \text{Cl}_2(g) \rightarrow 2\text{NOCl}(g) \]
A chemist proposes the following two-step mechanism for the reaction:
\[ \text{Step 1 (fast equilibrium):}\quad \text{NO}(g) + \text{Cl}_2(g) \underset{k_{-1}}{\overset{k_1}{\rightleftharpoons}} \text{NOCl}_2(g) \]
\[ \text{Step 2 (slow):}\quad \text{NOCl}_2(g) + \text{NO}(g) \xrightarrow{k_2} 2\text{NOCl}(g) \]
Based on this mechanism, which of the following is the correct rate law expression for the overall reaction in terms of elementary rate constants and reactant concentrations?
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