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Consider the following reaction between nitrogen dioxide gas and carbon monoxide gas NO2 (g) + CO (g) → NO (g) + CO2 (g) The experimentally determined rate law for this reaction is Rate = k [NO2]². A possible reaction mechanism involves two steps as shown below NO2 (g) + NO2 (g)→ NO3 (g) + NO (g) Slow NO3 (g) + CO (g) → NO2 (g) + CO2 (g) Fast Are there any intermediates in the proposed mechanism? If present, identify them. Which is the rate-determining step in the mechanism - the 1st one or the 2nd one? Why? What is the rate law for the rate determining step based on its molecularity? What is the rate law for the mechanism? How does the rate law for the overall reaction match the experimental rate law?

Consider the following reaction between nitrogen dioxide gas and carbon monoxide gas NO2 (g) + CO (g) → NO (g) + CO2 (g) The experimentally determined rate law for this reaction is Rate = k [NO2]². A possible reaction mechanism involves two steps as shown below NO2 (g) + NO2 (g)→ NO3 (g) + NO (g) Slow NO3 (g) + CO (g) → NO2 (g) + CO2 (g) Fast Are there any intermediates in the proposed mechanism? If present, identify them. Which is the rate-determining step in the mechanism - the 1st one or the 2nd one? Why? What is the rate law for the rate determining step based on its molecularity? What is the rate law for the mechanism? How does the rate law for the overall reaction match the experimental rate law?

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter12: Kinetics
Section: Chapter Questions
Problem 4E: A study of the rate of dimerization of C4H6 gave the data shown in the table: 2C4H6C8H12 (a)...
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Problem 1 Consider the following reaction between nitrogen dioxide gas and carbon monoxide gas NO2 (g) + CO (g) → NO (g) + CO2 (g) The experimentally determined rate law for this reaction is Rate = k [NO2]². A possible reaction mechanism involves two steps as shown below NO2 (g) + NO2 (g)→ NO3 (g) + NO (g) Slow NO3 (g) + CO (g) → NO2 (g) + CO2 (g) Fast Are there any intermediates in the proposed mechanism? If present, identify them. Which is the rate-determining step in the mechanism – the 1st one or the 2nd one? Why? What is the rate law for the rate determining step based on its molecularity? What is the rate law for the mechanism? How does the rate law for the overall reaction match the experimental rate law?
Transcribed Image Text:Problem 1 Consider the following reaction between nitrogen dioxide gas and carbon monoxide gas NO2 (g) + CO (g) → NO (g) + CO2 (g) The experimentally determined rate law for this reaction is Rate = k [NO2]². A possible reaction mechanism involves two steps as shown below NO2 (g) + NO2 (g)→ NO3 (g) + NO (g) Slow NO3 (g) + CO (g) → NO2 (g) + CO2 (g) Fast Are there any intermediates in the proposed mechanism? If present, identify them. Which is the rate-determining step in the mechanism – the 1st one or the 2nd one? Why? What is the rate law for the rate determining step based on its molecularity? What is the rate law for the mechanism? How does the rate law for the overall reaction match the experimental rate law?
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