   # At 40°C, H 2 O 2 ( aq ) will decompose according to the following reaction: 2H 2 O 2 ( a q ) → 2H 2 O ( l ) + O 2 ( g ) The following data were collected for the concentration of H 2 O 2 at various times. Times(s) [H 2 O 2 ](mol/L) 0 1.000 2.16 × 10 4 0.500 4.32 × 10 4 0.250 a. Calculate the average rate of decomposition of H 2 O 2 between 0 and 2.16 × 10 4 s. Use this rate to calculate the average rate of production of O 2 ( g ) over the same time period. b. What are these rates for the time period 2.16 × 10 4 s to 4.32 × 10 4 s? ### Chemistry

10th Edition
Steven S. Zumdahl + 2 others
Publisher: Cengage Learning
ISBN: 9781305957404

#### Solutions

Chapter
Section ### Chemistry

10th Edition
Steven S. Zumdahl + 2 others
Publisher: Cengage Learning
ISBN: 9781305957404
Chapter 12, Problem 27E
Textbook Problem
756 views

## At 40°C, H2O2 (aq) will decompose according to the following reaction: 2H 2 O 2 ( a q ) → 2H 2 O ( l ) + O 2 ( g ) The following data were collected for the concentration of H2O2 at various times. Times(s) [H2O2](mol/L) 0 1.000 2.16 × 104 0.500 4.32 × 104 0.250 a. Calculate the average rate of decomposition of H2O2 between 0 and 2.16 × 104 s. Use this rate to calculate the average rate of production of O2(g) over the same time period.b. What are these rates for the time period 2.16 × 104 s to 4.32 × 104 s?

(a)

Interpretation Introduction

Interpretation: The decomposition reaction of H2O2 is given. The answers for each option using appropriate data from the given table are to be stated.

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.

### Explanation of Solution

Explanation

Given

Concentration of H2O2 at 0s is 1.000mol/L .

Concentration of H2O2 at 2.16×104s is 0.500mol/L .

The reaction that takes place is,

2H2O2(aq)2H2O(l)+O2(g)

The rate law for the above equation is written as,

Rate=12Δ[H2O2]Δt=12Δ[H2O]Δt=12Δ[O2]Δt (1)

Where,

• Δ[H2O2] is the average rate of consumption of H2O2 .
• Δ[H2O] is the average rate of production of H2O .
• Δ[O2] is the average rate of production of O2 .
• Δt is the average time.

The average rate of decomposition of H2O2 between 0 and 2.16×104s is calculated as,

AverageRate=FinalconcentrationInitialconcentrationFinaltimeInitialtime

Substitute the values of concentration of H2O2 at 0 and 2

(b)

Interpretation Introduction

Interpretation: The decomposition reaction of H2O2 is given. The answers for each option using appropriate data from the given table are to be stated.

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.

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