   # Calculate the standard free energy change for the oxidation of 1.00 mol of SO 2 (g) to form SO 3 (g) using values of Δ f G °. ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 18.7, Problem 2CYU
Textbook Problem
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## Calculate the standard free energy change for the oxidation of 1.00 mol of SO2(g) to form SO3(g) using values of ΔfG°.

Interpretation Introduction

Interpretation:

The standard free energy change for oxidation of one mole SO2(g) should be calculated using ΔfGo.

Concept introduction:

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

ΔrG°=fG°(products)-fG°(reactants)

### Explanation of Solution

The standard free energy change for the oxidation of SO2(g) is calculated below.

Given: Oxidation of 1molSO2(g) forms SO3(g)

The balanced reaction is SO2(g)+12O2(g)SO3(g).

The Appendix L was referred for the values of standard free energy.

SO2(g)+12O2(g)SO3(g)ΔfG°(kJ/mol)-300.130-371.04

ΔrG°=fG°(products)-fG°(reactants)

ΔrG°=[(1 mol SO3(g)/mol-rxn)Δ<

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