9. The rate law for the reaction shown below is rate = k[NO21². %3D NO2(g) + CO(g) →NO(g) + CO2(g) One possible mechanism is shown and below. (1) NO2(g) + NO2(g) →NO3(g)+NO(g) | [slow] (2) NO3(g) + CO(g) →NO2(g) + CO2(g) [fast] The following alternative mechanism has been proposed. (1) 2 NO2(g) →N2(g) + 2 O2(g) [slow] (2) 2 CO(g) + O2(g) →2 CO2(g) [fast] (3) N2(g) + O2(g) →2 NO(g) [fast] Are the mechanisms consistent with the rate law?

9. The rate law for the reaction shown below is rate = k[NO21². %3D NO2(g) + CO(g) →NO(g) + CO2(g) One possible mechanism is shown and below. (1) NO2(g) + NO2(g) →NO3(g)+NO(g) | [slow] (2) NO3(g) + CO(g) →NO2(g) + CO2(g) [fast] The following alternative mechanism has been proposed. (1) 2 NO2(g) →N2(g) + 2 O2(g) [slow] (2) 2 CO(g) + O2(g) →2 CO2(g) [fast] (3) N2(g) + O2(g) →2 NO(g) [fast] Are the mechanisms consistent with the rate law?

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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