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: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section: Chapter Questions
Problem 70QRT
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