   # A possible mechanism for the decomposition of hydrogen peroxide is H 2 O 2 → 2 OH H 2 O 2 + OH → H 2 O + HO 2 HO 2 + OH → H 2 O + O 2 Using your results from Exercise 37, specify which step is the rate-determining step. What is the overall balanced equation for the reaction? ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 11, Problem 60E
Textbook Problem
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## A possible mechanism for the decomposition of hydrogen peroxide is H 2 O 2   →   2 OH H 2 O 2   +   OH →   H 2 O   +   HO 2 HO 2   +   OH →   H 2 O   +   O 2 Using your results from Exercise 37, specify which step is the rate-determining step. What is the overall balanced equation for the reaction?

Interpretation Introduction

Interpretation: A proposed mechanism of decomposition of hydrogen peroxide is given. The rate determining step and overall balanced equation for the reaction is to be determined.

Concept introduction: The change observed in the concentration of a reactant or a product per unit time is known as the rate of the particular reaction. The differential rate law provides the rate of a reaction at specific reaction concentrations.

To determine: The rate determining step for the decomposition of hydrogen peroxide.

### Explanation of Solution

The decomposition of hydrogen peroxide is first order reaction. The given reaction consists of only one reactant, that is, H2O2 . Hence, the rate law for the given reaction is,

Rate=k[H2O2]

The slow step of reaction mechanism is rate determining step. In the given mechanism of a reaction, first step is slow step. Hence, it is a rate determining step, that is,

H2O22OH

To determine: The overall balanced equation of the given reaction.

The first step in proposed mechanism is,

H2O22OH

The second step in proposed mechanism is,

H2O2+OHH2O+HO

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