Chapter 15.5, Problem 15.6CYU

### Chemistry & Chemical Reactivity

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

Chapter
Section

### 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)â€‰â€‰â€‰â‡„â€‰â€‰2O3(g)â€‰â€‰

The equilibrium constant can be written as,

Kâ€‰â€‰=â€‰â€‰[O3]â€‰â€‰[O2]3/2â€‰

K1â€‰=â€‰[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

### Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

#### The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started