   Chapter 18, Problem 38PS

Chapter
Section
Textbook Problem

For the reaction TiCl2(s) + Cl2(g) → TiCl4(ℓ), ΔrG° = −272.8 kj/mol-txn. Using this value and other data available in Appendix L, calculate the value of ΔfG° for TiCl2(s).

Interpretation Introduction

Interpretation:

The value of ΔfG° for TiCl2(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 TiCl2(s) is calculated below.

Given:

The standard free energy change value of TiCl4(l) is 737.2 kJ/mol.

The standard free energy change value of Cl2(g) is 0 kJ/mol.

The given reaction is,

TiCl2(s)+Cl2(g)TiCl4(l)

The ΔrG° for the reaction is 272.8 kJ/mol-rxn.

The expression for the free energy change is:

ΔrG°=nΔfG°(products)nΔfG°(reactants)=[(1 mol TiCl4(l)/mol-rxn)ΔfG°[TiCl4(l)][(1 mol TiCl2(

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