AP Chemistry
5.11 Catalysis
5.8 Reaction Mechanism and Rate Law
5.7 Introduction to Reaction Mechanisms
The decomposition of hydrogen peroxide, \(\text{H}_2\text{O}_2\text{(aq)}\), is catalyzed by iodide ions, \(\text{I}^-\text{(aq)}\), according to the overall reaction:
\[ 2\text{ H}_2\text{O}_2\text{(aq)} \rightarrow 2\text{ H}_2\text{O}\text{(l)} + \text{O}_2\text{(g)} \]
Kinetic measurements demonstrate that the reaction is first order with respect to \(\text{H}_2\text{O}_2\) and first order with respect to \(\text{I}^-\), giving the experimental rate law:
\[ \text{Rate} = k [\text{H}_2\text{O}_2][\text{I}^-] \]
Which of the following proposed mechanisms is consistent with both the overall balanced equation and the experimental rate law?
\[ 2\text{ H}_2\text{O}_2\text{(aq)} \rightarrow 2\text{ H}_2\text{O}\text{(l)} + \text{O}_2\text{(g)} \]
Kinetic measurements demonstrate that the reaction is first order with respect to \(\text{H}_2\text{O}_2\) and first order with respect to \(\text{I}^-\), giving the experimental rate law:
\[ \text{Rate} = k [\text{H}_2\text{O}_2][\text{I}^-] \]
Which of the following proposed mechanisms is consistent with both the overall balanced equation and the experimental rate law?
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