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The gas-phase decomposition of ozone is thought to occur by the following two-step mechanism. Step 1 : O3(g) ⟹O2(g) O(g) (fast) Step 2 : O(g) O3(g) ⟶ 2 O2(g) ( slow ) (a) Write the balanced equation for the overall reaction. (b) Derive the rate law that is consistent with this mechanism. (Hint: The product appears in the rate law.) (c) Is O a catalyst or an intermediate? (d) If instead the reaction occurred in a single step, would the rate law change? If so, what would it be? |
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