   Chapter 18, Problem 46PS

Chapter
Section
Textbook Problem

The standard free energy change, ΔrG°, for the formation of O3(g) from O2(g) is +163.2 kJ/mol-rxn at 25 °C. Calculate Kp at this temperature for the equilibrium3 O2(g) ⇄ 2 O3(g)Comment on the sign of ΔrG° and the magnitude of Kp.

Interpretation Introduction

Interpretation:

The equilibrium constant for the given reaction should be calculated. The sign of ΔrG° and magnitude of Kp should be explained.

Concept introduction:

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by ΔrG. It can be calculated in a similar manner as entropy and enthalpy.  The expression for the free energy change is:

ΔrG°=nΔfG°(products)nΔfG°(reactants)

ΔG is related to the equilibrium constant K by the equation,

ΔrG=RTlnKp.

The rearranged expression is,

Kp=eΔrGRT

Explanation

The equilibrium constant for the given reaction of formation of O3(g) is calculated below.

Given:

The given reaction is,

3O2(g)2O3(g)

The ΔrG value for the reaction is +163.2 kJ/mol- rxn at 298.15 K.

ΔG is related to the equilibrium constant K by the equation,

ΔrG=RTlnKp.

The rearranged expression is,

Kp=eΔrGRT

Substitute the value of ΔrG°, T and R

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

Find more solutions based on key concepts 