can you help w/ d? ### Chemical Reaction Mechanism and Rate Law Analysis#### c. Analysis of a Proposed MechanismA possible mechanism for the given reaction consists of two steps:\[ \text{NO}_2(\text{g}) + \text{NO}_2(\text{g}) \rightarrow \text{NO}_3(\text{g}) + \text{NO}(\text{g}) \quad \text{[slow]} \]\[ \text{NO}_3(\text{g}) + \text{CO}(\text{g}) \rightarrow \text{NO}_2(\text{g}) + \text{CO}_2(\text{g}) \quad \text{[fast]} \]**Question:** Is this proposed mechanism consistent with the experimentally determined rate law? Explain.#### d. Identifying the Reaction Intermediate**Question:** What is the reaction intermediate in the proposed mechanism?---### Explanation**Section c:** The proposed mechanism comprises two steps: the first step is slow, involving the reaction of two nitrogen dioxide \((\text{NO}_2)\) molecules to form nitrogen trioxide \((\text{NO}_3})\) and nitrogen monoxide \((\text{NO})\). The second, faster step involves the reaction of \(\text{NO}_3\) with carbon monoxide \((\text{CO})\) to produce \(\text{NO}_2}\) and carbon dioxide \((\text{CO}_2})\).To determine consistency with the experimentally determined rate law, one needs to:- Derive the rate law from the slow step (since it is the rate-determining step).- Compare this derived rate law with the experimentally determined rate law to check for consistency.**Section d:** The reaction intermediate is a molecule that is produced in one step of the reaction mechanism and consumed in a subsequent step. In this proposed mechanism, \(\text{NO}_3}\) is produced in the first step and consumed in the second step, thus it is the reaction intermediate.---Understanding and analyzing the proposed mechanism helps in verifying its consistency with the experimental observations and further elucidates the steps involved in the chemical reaction.

The speed at which a chemical reaction takes place is called the rate of the reaction. It depends…

c. A possible mechanism for this reaction involves two steps: NO2(g) + NO2(g) - NO3(g) + NO(g) slow NO3(g) + CO(g) → NO2(g) + CO2(g) fast Is this proposed mechanism consistent with the experimentally determined rate law? Explain. d. What is the reaction intermediate in the proposed mechanism?

c. A possible mechanism for this reaction involves two steps: NO2(g) + NO2(g) - NO3(g) + NO(g) slow NO3(g) + CO(g) → NO2(g) + CO2(g) fast Is this proposed mechanism consistent with the experimentally determined rate law? Explain. d. What is the reaction intermediate in the proposed mechanism?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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