**Question 2**The decomposition of hydrogen peroxide is catalyzed by iodide in a two-step process:1. \( \text{H}_2\text{O}_2 + \text{I}^- \rightarrow \text{H}_2\text{O} + \text{IO}^- \) (slow)2. \( \text{IO}^- + \text{H}_2\text{O}_2 \rightarrow \text{H}_2\text{O} + \text{O}_2 + \text{I}^- \) (fast)Overall reaction:\[ \underline{2\text{H}_2\text{O}_2 \rightarrow 2\text{H}_2\text{O} + \text{O}_2} \]**What is the rate law predicted by this mechanism?**- ○ Rate = k[\(\text{H}_2\text{O}_2\)]- ○ Rate = k[\(\text{H}_2\text{O}_2\)][\(\text{I}^-\)]- ○ Rate = k[\(\text{H}_2\text{O}_2\)]^2- ○ Rate = k[\(\text{H}_2\text{O}_2\)][\(\text{IO}^-\)]

QUESTION 2 The decomposition of hydrogen peroxide is catalyzed by iodide in a two-step process: H202 +I-H20 + IO- I0- +H202-H20+ O2 +I- (slow) (fast) 2H202 -2H20 + 02 What is the rate law predicted by this mechanism? Rate = k[H2O2] Rate = k[H2O2][I %3D %3D Rate = k[H2O22 Rate = k[H2O2][I0] %3D

QUESTION 2 The decomposition of hydrogen peroxide is catalyzed by iodide in a two-step process: H202 +I-H20 + IO- I0- +H202-H20+ O2 +I- (slow) (fast) 2H202 -2H20 + 02 What is the rate law predicted by this mechanism? Rate = k[H2O2] Rate = k[H2O2][I %3D %3D Rate = k[H2O22 Rate = k[H2O2][I0] %3D

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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Expert Solution

Step 1

Rate of reaction depends on slow step reaction, because it is a rate determining step.

H2O2 + I ➡️ H2O + IO-

So rate of reaction depends on concentration of reactants of slow step reaction.

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