The gas-phase decomposition of ozone is thought to oc- cur by the following two-step mechanism. Step 1: 03(8) = 02(8) + O(g) (fast) Step 2: 0(8) + O,(8) → 202(8) (slow) (a) Write the balanced equation for the overall reaction. (b) Derive the rate law that is consistent with this mecha- nism. (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?
The gas-phase decomposition of ozone is thought to oc- cur by the following two-step mechanism. Step 1: 03(8) = 02(8) + O(g) (fast) Step 2: 0(8) + O,(8) → 202(8) (slow) (a) Write the balanced equation for the overall reaction. (b) Derive the rate law that is consistent with this mecha- nism. (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?
Chapter13: Kinetic Methods
Section: Chapter Questions
Problem 3P
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