   # One of the reactions that destroys ozone in the upper atmosphere is NO ( g ) + O 3 ( g ) ⇌ NO 2 ( g ) + O 2 ( g ) Using data from Appendix 4, calculate ∆G ° and K (at 298 K) for this 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 16, Problem 69E
Textbook Problem
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## One of the reactions that destroys ozone in the upper atmosphere is NO ( g ) + O 3 ( g ) ⇌ NO 2 ( g ) + O 2 ( g ) Using data from Appendix 4, calculate ∆G° and K (at 298 K) for this reaction.

Interpretation Introduction

Interpretation: The reaction that destroys ozone in the upper atmosphere is given. The value of ΔG° and K at given temperature is to be calculated.

Concept introduction: Equilibrium constant, K , is the measure of concentration of reactants and products of a system at equilibrium. If the reaction is at equilibrium, the free energy change,

ΔG=0Q=K

ΔG=ΔG°+RTln(Q)

### Explanation of Solution

The reaction that takes place is,

NO(g)+O3(g)NO2(s)+O2(g)

Refer to Appendix 4 .

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

 Molecules ΔG°(kJ/mol) NO2(g) 52 O2(g) 0 NO(g) 87 O3(g) 163

The formula of ΔG° is,

ΔG°=npΔG°(product)nfΔG°(reactant)

Where,

• np is number of moles of each product.
• nr is number of moles each reactant.
• ΔG°(product) is free energy of product at a pressure of 1atm .
• ΔG°(reactant) is free energy of reactant at a pressure of 1atm .

Substitute all values from the table in the above equation.

ΔG°=npΔG°(product)nfΔG°(reactant)=[1(52)+0(229){(87)(163)}]kJ=198kJ_

The value of ΔG° is 198kJ

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