Chapter 9, Problem 9.76EP

### General, Organic, and Biological C...

7th Edition
H. Stephen Stoker
ISBN: 9781285853918

Chapter
Section

### General, Organic, and Biological C...

7th Edition
H. Stephen Stoker
ISBN: 9781285853918
Textbook Problem

# Calculate the value of the equilibrium constant for the reaction N 2 ( g ) + 2 O 2 ( g ) ⇌ 2 NO 2 ( g ) if the concentrations of the species at equilibrium are [N2] = 0.0013, [O2] = 0.0024, and [NO2] = 0.00065.

Interpretation Introduction

Interpretation:

The value of equilibrium constant for the equation has to be calculated.

N2(g) + 2O2(g)  2NO2(g)

Concept Introduction:

Law of Chemical Equilibrium:

The equilibrium constant is the product of molar concentrations of the product which is raised to its stoichiometric coefficients divided by the product of molar concentrations of the reactant which is raised to its stoichiometric coefficients.

Equilibrium Constant:

Consider a reaction,

aA+bBcC+dD

Forward reaction rate Kf= [A]a[B]B

Backward reaction rate Kb= [C]c[D]d

At equilibrium, the rate of forward reaction = rate of backward reaction

Keq=KfKb KfKb=[C]c[D]d[A]a[B]B

Keq=KfKb=[C]c[D]d[A]a[B]B

Keq is the equilibrium constant.

Explanation

The given equation is:

Â Â Â Â N2(g)Â +Â 2O2(g)Â â‡ŒÂ 2NO2(g)

The equilibrium constant Keq=[NO2]2[N2][O2]2â†’eq(1)

Given,

Â Â Â Â [NO2]Â =Â 0

### 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