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Consider the mechanism. Step 1: Step 2: Overall: A B+C C+D E - equilibrium slow A+DB+E Determine the rate law for the overall reaction, where the overall rate constant is represented as k.

Consider the mechanism. Step 1: Step 2: Overall: A B+C C+D E - equilibrium slow A+DB+E Determine the rate law for the overall reaction, where the overall rate constant is represented as k.

Chemistry
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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Consider the mechanism. **Step 1:** \[ \text{A} \rightleftharpoons \text{B} + \text{C} \] (equilibrium) **Step 2:** \[ \text{C} + \text{D} \rightarrow \text{E} \] (slow) **Overall:** \[ \text{A} + \text{D} \rightarrow \text{B} + \text{E} \] **Determine the rate law for the overall reaction, where the overall rate constant is represented as \( k \).** In this mechanism, Step 1 is at equilibrium, which means the forward and reverse reactions occur at the same rate. Step 2 is slow, indicating it is the rate-determining step. To write the rate law, consider the slow step. To derive the overall rate law, we can use the concentration of the intermediate \( \text{C} \), determined from the equilibrium step, to express the rate law in terms of the initial reactants \( \text{A} \) and \( \text{D} \).
Transcribed Image Text:Consider the mechanism. **Step 1:** \[ \text{A} \rightleftharpoons \text{B} + \text{C} \] (equilibrium) **Step 2:** \[ \text{C} + \text{D} \rightarrow \text{E} \] (slow) **Overall:** \[ \text{A} + \text{D} \rightarrow \text{B} + \text{E} \] **Determine the rate law for the overall reaction, where the overall rate constant is represented as \( k \).** In this mechanism, Step 1 is at equilibrium, which means the forward and reverse reactions occur at the same rate. Step 2 is slow, indicating it is the rate-determining step. To write the rate law, consider the slow step. To derive the overall rate law, we can use the concentration of the intermediate \( \text{C} \), determined from the equilibrium step, to express the rate law in terms of the initial reactants \( \text{A} \) and \( \text{D} \).
Expert Solution
Step 1

Given -

Step-1.          A <-> B + C (equilibrium)

Step-2.           C + D ->  E (slow) 

Overall            A + D  -> B + E

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