Consider the oxidation of nitrogen monoxide with the observed rate law below. Rate = k(No)°C02J %3D 2 NO (g)+ O2cg) →2N2 (g) The proposed two-step mechanism is: I. NO (g) + Oz ( = NO3 NO 3 cg) (Fast, reversible) I NO3 c9) + NO lg) → 2 NO2 (9) (Slow) D. Write rate laws for the elementary steps. Give the molecularity for each step. E. Using rate laws from part d., determine a reasonable rate law for the overall process, including values for reaction orders. Is the mechanism reasonable and consistent with the observed rate law? Fully explain and show ALL work.

Consider the oxidation of nitrogen monoxide with the observed rate law below. Rate = k(No)°C02J %3D 2 NO (g)+ O2cg) →2N2 (g) The proposed two-step mechanism is: I. NO (g) + Oz ( = NO3 NO 3 cg) (Fast, reversible) I NO3 c9) + NO lg) → 2 NO2 (9) (Slow) D. Write rate laws for the elementary steps. Give the molecularity for each step. E. Using rate laws from part d., determine a reasonable rate law for the overall process, including values for reaction orders. Is the mechanism reasonable and consistent with the observed rate law? Fully explain and show ALL work.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter18: Chemical Kinetics

Section: Chapter Questions

Problem 70AP

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