**Reaction Mechanism Explanation:**Consider the following reaction mechanism. If this mechanism is correct, and \( k_1 \) is much smaller than \( k_2 \), then the observed rate law would be:1. **Reaction Step 1:** \[ 2A \xrightarrow{k_1} C + I \]2. **Reaction Step 2:** \[ I + B \xrightarrow{k_2} C + D \]**Choices for the Observed Rate Law:**- \( R = k_1 [A]^2 \)- \( R = k_1 k_2 [A]^2 [I] [B] \)- \( R = k_1 [A]^2 - k_2 [C] [D] \)- \( R = k_1 [A] \)- \( R = k_2 [I] [B] \)**Explanation:**The mechanism consists of two steps. In the first step, two molecules of A react to give species C and an intermediate I, with the rate constant \( k_1 \). In the second step, the intermediate I reacts with B to produce species C and D, with the rate constant \( k_2 \).Since \( k_1 \) is much smaller than \( k_2 \), the first step is likely the rate-determining step. The observed rate law will depend on the concentration of reactants involved in this slowest step.

Step : 1 The correct option for the following mechanism is follows as :

Answered: Consider the following reaction…

Consider the following reaction mechanism. If this mechanism is correct, and ki is much smaller than k2, then the observed rate law would be: ki 2 A C + I k2 I + B C + D

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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Question

**Reaction Mechanism Explanation:**

Consider the following reaction mechanism. If this mechanism is correct, and \( k_1 \) is much smaller than \( k_2 \), then the observed rate law would be:

1. **Reaction Step 1:**

\[
2A \xrightarrow{k_1} C + I
\]

2. **Reaction Step 2:**

\[
I + B \xrightarrow{k_2} C + D
\]

**Choices for the Observed Rate Law:**

- \( R = k_1 [A]^2 \)
- \( R = k_1 k_2 [A]^2 [I] [B] \)
- \( R = k_1 [A]^2 - k_2 [C] [D] \)
- \( R = k_1 [A] \)
- \( R = k_2 [I] [B] \)

**Explanation:**

The mechanism consists of two steps. In the first step, two molecules of A react to give species C and an intermediate I, with the rate constant \( k_1 \). In the second step, the intermediate I reacts with B to produce species C and D, with the rate constant \( k_2 \).

Since \( k_1 \) is much smaller than \( k_2 \), the first step is likely the rate-determining step. The observed rate law will depend on the concentration of reactants involved in this slowest step.

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