   # Use bond energies to estimate the maximum wavelength light that will cause the reaction O 3 → h v O 2 + O ### 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 19, Problem 53E
Textbook Problem
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## Use bond energies to estimate the maximum wavelength light that will cause the reaction O 3 → h v O 2 + O

Interpretation Introduction

Interpretation: The reaction corresponding to the decomposition of O3 is given. The value of maximum wavelength of light is to be calculated for this reaction using bond energy values.

Concept introduction: The expression to calculate the wavelength of light is,

E=hcλλ=hcE

To determine: The value of maximum wavelength of light is calculated for the given reaction using the bond energies.

### Explanation of Solution

Explanation

The stated reaction is,

O3hvO2+O

Refer to Table 3-3 .

The value of bond energy, D°(kJ/mol) , for the given reactant and product is,

 Bonds D°(kJ/mol) O=O(in O2) 0 O−O 146 O=O(in O3) 0

The formula of ΔH° is,

ΔH°=npD°(bondsbroken)nfD°(bondsformed)

Where,

• np is number of moles of each product.
• nr is number of moles each reactant.
• D°(bonds broken) is the bond energy of broken bonds.
• D°(bondsformed) is the bond energy of bonds formed.

Substitute all values from the table in the above equation.

ΔH°=npD°(bondsbroken)nfD°(bondsformed)=(1×DO=O+1×DOO)(1×DO=O)=[(1×0)+(1×146)(1×0)]kJ

Simplify the above equation.

ΔH°=[(1×0)+(1×146)(1×0)]kJ=146kJ_

The required value of energy to break one bond is 2.42×1019J_ .

The required energy for the reaction to occur is 146kJ .

The conversion of kilo-joule (kJ) into joule (J) is done as,

1kJ=103J

Hence,

The conversion of 146.0kJ into joule is,

146

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