6. The rate law for the overall reaction 2 N2O5 (g) →4 NO2 (g) + O2 (g) is Rate = k[N2Os). a. Consider this mechanism: N2Os (g) → NO3 (g) + NO2 (g) (fast) NO2 (g) + N2Os (g)→ 3 NO2 (g) + 02 (g) (fast] i. ii. (slow] i. NO3 (g) +0 (g) – NO2 (g) + O2 (g) Is this reaction mechanism consistent with the rate law? Why or Why not? b. If the reaction mechanism is not consistent with the rate law, how would it need to change to become consistent? c. List potential reaction intermediates present in this mechanism. d. Draw a reaction energy diagram for this mechanism including any modifications you've made in a-c.

6. The rate law for the overall reaction 2 N2O5 (g) →4 NO2 (g) + O2 (g) is Rate = k[N2Os). a. Consider this mechanism: N2Os (g) → NO3 (g) + NO2 (g) (fast) NO2 (g) + N2Os (g)→ 3 NO2 (g) + 02 (g) (fast] i. ii. (slow] i. NO3 (g) +0 (g) – NO2 (g) + O2 (g) Is this reaction mechanism consistent with the rate law? Why or Why not? b. If the reaction mechanism is not consistent with the rate law, how would it need to change to become consistent? c. List potential reaction intermediates present in this mechanism. d. Draw a reaction energy diagram for this mechanism including any modifications you've made in a-c.

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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