Chapter 18, Problem 18.86QP

Interpretation Introduction

Interpretation:

The mole fractions of $(CO)$ and $(C{O}_2)$ at equilibrium should be calculated under given conditions.

Concept Introduction:

Free energy (Gibbs free energy) is the term that is used to explain the total energy content in a thermodynamic system that can be converted into work.  The free energy is represented by the letter $\text{G}$.  All spontaneous process is associated with the decrease of free energy in the system.  The standard free energy change ${\text{(ΔG}}^{\text{°}}{}_{\text{rxn}})$ is the difference in free energy of the reactants and products in their standard state.

${\text{ΔG}}^{\text{°}}{}_{\text{rxn}}\text{=}\sum {\text{nΔG}}_{\text{f}}{}^{\text{°}}\text{(Products)-}\sum {\text{nΔG}}_{\text{f}}{}^{\text{°}}\text{(Reactants)}$

Mole fraction:

Mole fraction ($X$) of any compound in a solution is the number of moles of the component divided by total number of moles making up a solution. It is denoted by $X$

  $Molefraction(X)=\frac{Molesofcomponent}{\begin{array}{l}Totalnumberofmoles\\ makingupthesolutions\end{array}}$