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8. For the overall reaction: 2NO (g) +O2 (g) → 2NO2 (g), the following mechanism has been proposed: (1) 2NO (g) = N2O2 (g) (2) N2O2 (g) + O2 (g) → 2 NO2 (g) a) Determine the rate law expression for this reaction. The steady-state approximation can be used for the N2O2 intermediate. b) Simplify the rate law expression if the rate constant for reaction (2) is much larger than that for the reverse reaction (1).

8. For the overall reaction: 2NO (g) +O2 (g) → 2NO2 (g), the following mechanism has been proposed: (1) 2NO (g) = N2O2 (g) (2) N2O2 (g) + O2 (g) → 2 NO2 (g) a) Determine the rate law expression for this reaction. The steady-state approximation can be used for the N2O2 intermediate. b) Simplify the rate law expression if the rate constant for reaction (2) is much larger than that for the reverse reaction (1).

Chemistry: The Molecular Science
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
Section11.7: Reaction Mechanisms
Problem 11.12E
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8. For the overall reaction: 2NO (g) + O2 (g) → 2NO2 (g), the following mechanism has been proposed: (1) 2NO (g) = N2O2 (g) (2) N2O2 (g) + O2 (g) → 2 NO2 (g) a) Determine the rate law expression for this reaction. The steady-state approximation can be used for the N2O2 intermediate. b) Simplify the rate law expression if the rate constant for reaction (2) is much larger than that for the reverse reaction (1).
Transcribed Image Text:8. For the overall reaction: 2NO (g) + O2 (g) → 2NO2 (g), the following mechanism has been proposed: (1) 2NO (g) = N2O2 (g) (2) N2O2 (g) + O2 (g) → 2 NO2 (g) a) Determine the rate law expression for this reaction. The steady-state approximation can be used for the N2O2 intermediate. b) Simplify the rate law expression if the rate constant for reaction (2) is much larger than that for the reverse reaction (1).
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