The decomposition of ozone, , follows the mechanism: Step 1: (fast equilibrium, forward, backward); Step 2: (slow, ). Using the rapid equilibrium assumption, the correct effective rate law is:

Question

The decomposition of ozone, $2O_3 \rightarrow 3O_2$, follows the mechanism: Step 1: $O_3 \rightleftharpoons O_2 + O$ (fast equilibrium, $k_1$ forward, $k_{-1}$ backward); Step 2: $O + O_3 \rightarrow 2O_2$ (slow, $k_2$). Using the rapid equilibrium assumption, the correct effective rate law is:

Prashant Kotian · Accepted Answer

Correct answer: A. The rate determining step is the slow step: . Since atomic oxygen () is an intermediate, we apply equilibrium to the fast step: . Substituting this intermediate concentration into the RDS gives: .

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