4.) The overall reaction 2NO2(g) + F2(g) →2NO2F(g) has an experimental rate law Rate = k[NO2][F2]. The accepted two step mechanism is: %3D (1) NO2(g) + F2(g) → NO2F(g) + F(g) (2) NO2(g) + F(g) → NO,F(g) [slow; rate determining] [fast] a. Write the rate laws for each of the elementary steps. b. What is the molecularity for each step? C. Show how the elementary steps sum to the overall balanced equation: d. Which species (if any) are intermediates? Which step is rate-limiting? e. f. Is the mechanism reasonable and consistent with the observed rate law? Explain

4.) The overall reaction 2NO2(g) + F2(g) →2NO2F(g) has an experimental rate law Rate = k[NO2][F2]. The accepted two step mechanism is: %3D (1) NO2(g) + F2(g) → NO2F(g) + F(g) (2) NO2(g) + F(g) → NO,F(g) [slow; rate determining] [fast] a. Write the rate laws for each of the elementary steps. b. What is the molecularity for each step? C. Show how the elementary steps sum to the overall balanced equation: d. Which species (if any) are intermediates? Which step is rate-limiting? e. f. Is the mechanism reasonable and consistent with the observed rate law? Explain

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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