Chapter 18, Problem 37PS

### 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

# For the reaction BaCO3(s) → BaO(s) + CO2(g), ΔrG° = +219.7 kJ/mol-rxn. Using this value and other data available in Appendix L, calculate the value of ΔfG° for BaCO3(s).

Interpretation Introduction

Interpretation:

The value of ΔfG° for BaCO3(s) should be calculated.

Concept introduction:

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by ΔG. 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)

Explanation

The value of ΔfG° for BaCO3(s) is calculated below.

Given:

The standard free energy change value of BaO(s) is 520.38 kJ/mol.

The standard free energy change value of CO2(g) is 394.359 kJ/mol.

The given reaction is,

BaCO3(s)BaO(s)+CO2(g)

The ΔrG° for the reaction is +219.7 kJ/mol-rxn.

The expression for the free energy change is:

ΔrG°=nΔfG°(products)nΔfG°(reactants)=[[(1 mol BaO(s)/mol-rxn)ΔfG°[BaO(s)]+(1 mol CO2(g)/mol-rxn

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