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?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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