For the reaction, NO₂(g) + CO(g) → NO(g) +CO₂(g), the experimentally determined rate law is, Rate = K[NO₂]². A suggested mechanism for this reaction is, step 1: NO₂(g) + NO2(g) → NO3(g) + NO(g) step 2: NO3(g) + CO(g) → NO₂(g) + CO₂(g) a. Write the rate law for each elementary step in the reaction. b. Is this a reasonable mechanism for this reaction? Why or why not? c. Which step is the slow step in this mechanism? Why? d. Identify any intermediates in the reaction.

For the reaction, NO₂(g) + CO(g) → NO(g) +CO₂(g), the experimentally determined rate law is, Rate = K[NO₂]². A suggested mechanism for this reaction is, step 1: NO₂(g) + NO2(g) → NO3(g) + NO(g) step 2: NO3(g) + CO(g) → NO₂(g) + CO₂(g) a. Write the rate law for each elementary step in the reaction. b. Is this a reasonable mechanism for this reaction? Why or why not? c. Which step is the slow step in this mechanism? Why? d. Identify any intermediates in the reaction.

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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