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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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Chapter
Section
BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

The conversion of oxygen to ozone has a very small equilibrium constant.

3/2 O2(g) ⇄ O3(g) K = 2.5 × 10−29

(a) What is the value of K when the equation is written using whole-number coefficients?

3 O2(g) ⇄ 2 O3(g)

(b) What is the value of K for the conversion of ozone to oxygen?

2 O3(g) ⇄ 3 O2(g)

(a)

Interpretation Introduction

Interpretation: The equilibrium constant for the balanced equation has to be identified.

Concept Introduction: At equilibrium the concentration of the reaction and the product is equated to a constant K, where K is known as the equilibrium

If a reaction is as aA+bBcC+dD ,

The equilibrium constant K=[C]c[D]d[A]a[B]b

Explanation

For the reaction, 3O2(g)2O3(g)

The equilibrium constant can be written as,

K=[O3][O2]3/2

K1=[O3]2

(b)

Interpretation Introduction

Interpretation: The equilibrium constant for the conversion of ozone to oxygen has to be identified.

Concept Introduction: At equilibrium the concentration of the reaction and the product is equated to a constant K, where K is known as the equilibrium

If a reaction is as aA+bBcC+dD ,

The equilibrium constant K=[C]c[D]d[A]a[B]b

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