Chapter 17, Problem 17.107SP

Interpretation Introduction

Interpretation:

ΔG for formation of solid UF6 has to be calculated and it has to be determined if the reaction is spontaneous in forward or reverse direction.

Concept Introduction:

Gibbs free energy of formation is the change in Gibbs free energy associated with the formation of one mole of the compound from its components in their standard states. Mathematically it is defined as shown below:

$\Delta \text{G}\circ \left(\text{rxn}\right)=\Sigma \Delta \text{G}\circ \text{f}(\text{products})-\Sigma \Delta \text{G}\circ \text{f}(\text{reactants})$

The spontaneity of a reaction can be measured by the sign of Gibbs Free Energy. If Gibbs Free Energy is NEGATIVE then the reaction is spontaneous and vice -versa.

The free energy change for the reaction at non-standard state conditions can be calculated using the following formulae:

$\Delta \text{G }=\Delta \text{G}°+\text{ RT ln Q}$ ; Where Q is the reaction quotient

To determine:

ΔG for formation of solid and check spontanity of reaction.

Given:

The standard free- energy of formation of UF6 = -2068 kJ/mol