   Chapter 12, Problem 60E

Chapter
Section
Textbook Problem

# 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

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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