The oxidation of NO(g) to NO2(g): 2 NO(g) + O2(g) kobs 2 NO2(g) A mechanism of steps (a) - (c) is proposed below, all steps are elementary: k3 (a) NO(g) + NO(g) N2O2(g) k-3 (b) N2O2(g) → NO(g) + NO(g) k4 (c) N2O2(g) + O2(g) 2 NO2(g) Apply the steady-state approximation, find out the reaction rate law when the initial concertation of [O2] is high. Which step is rate-determining?

The oxidation of NO(g) to NO2(g): 2 NO(g) + O2(g) kobs 2 NO2(g) A mechanism of steps (a) - (c) is proposed below, all steps are elementary: k3 (a) NO(g) + NO(g) N2O2(g) k-3 (b) N2O2(g) → NO(g) + NO(g) k4 (c) N2O2(g) + O2(g) 2 NO2(g) Apply the steady-state approximation, find out the reaction rate law when the initial concertation of [O2] is high. Which step is rate-determining?

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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