Chapter 18.6, Problem 18.7CYU

### 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

# Determine the value of ΔrG° for the reaction C(s) + CO2(g) ⇄ 2 CO(g) from data in Appendix L. Use this result to calculate the equilibrium constant.

Interpretation Introduction

Interpretation:

The value of ΔrG° for given reaction C(s) + CO2(g)2CO(g) should be determined which then used to calculate the equilibrium constant for the reaction.

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°fG°(products)fG°(reactants)

ΔrG° is related to the equilibrium constant K by the equation,

ΔrGo= - RTlnKp.

The rearranged expression required to calculate equilibrium constant from ΔrG° is as follows,

Kp= e-ΔrGoRT

Explanation

The ΔrG° and the equilibrium constant for the given reaction is calculated as follows,

Given: C(s) + CO2(g)2CO(g)

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

The given reaction is,

C(s) + CO2(g)2CO(g)

The ΔrG° for C(s) is 0 kJ/mol

The ΔrG° for CO2(g) is -394.36 kJ/mol

The ΔrG° for CO(g) is -137.17 kJ/mol

ΔrG°fG°(products) -fG°(reactants)

ΔrG°[(2 mol CO(g)/mol-rxn)ΔfG°[CO(g)]-[(1 mol CO2(g)/mol-rxn)Δ

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