Chapter 5, Problem 57P

(a)

Interpretation Introduction

Interpretation:

Change in $\Delta G^0$ with the given $K_{eq}$ values should be determined.

Concept introduction:

Gibbs free energy change $\Delta G^0$: The difference between the free energy of the products and the free energy of reactants under standard conditions is called Gibbs free energy change.

Gibbs free energy change $\Delta G^0$ can be formulated in terms of enthalpy, entropy and temperature as,

$\begin{array}{l}{\text{ΔG}}^{\text{0}}\text{=}{\text{ΔH}}^{\text{0}}\text{-}{\text{TΔS}}^{\text{0}}\\ {\text{ΔH}}^{\text{0}}\text{is}\text{the}\text{standard}\text{enthalpy}\text{change}\\ {\text{ΔS}}^{\text{0}}\text{is}\text{the}\text{standard}\text{entropy}\text{change}\end{array}$

Equilibrium constant: The relative concentration of reactants and products at equilibrium can be expressed by equilibrium constant.

For a general reaction $A+B\rightleftarrows C+D$

$K_{eq}=\frac{\left[\mathrm{Pr}oducts\right]}{\left[\mathrm{Re}actnts\right]}=\frac{\left[C\right]\left[D\right]}{\left[A\right]\left[B\right]}$

Gibbs free energy change: The difference between the free energy of the products and the free energy of reactants under standard conditions is called Gibbs free energy change.

$\begin{array}{l}{\text{ΔG}}^{\text{0}}\text{=}\text{-RT}\text{ln}{\text{K}}_{\text{eq}}\\ \text{R}\text{is}\text{the}\text{gas}\text{constant}\\ \text{T}\text{is}\text{the}\text{temperature}\text{in}\text{K}\\ {\text{K}}_{\text{eq}}\text{is}\text{the}\text{equilibrium}\text{constant}\end{array}$

(b)

Interpretation Introduction

Interpretation:

The variation of $\Delta H^0$ if $\Delta S^0=0kcalmo{l}^{-1}{K}^{-1}$ should be determined.

 Concept introduction:

Gibbs free energy change $\Delta G^0$: The difference between the free energy of the products and the free energy of reactants under standard conditions is called Gibbs free energy change.

Gibbs free energy change $\Delta G^0$ can be formulated in terms of enthalpy, entropy and temperature as,

$\begin{array}{l}{\text{ΔG}}^{\text{0}}\text{=}{\text{ΔH}}^{\text{0}}\text{-}{\text{TΔS}}^{\text{0}}\\ {\text{ΔH}}^{\text{0}}\text{is}\text{the}\text{standard}\text{enthalpy}\text{change}\\ {\text{ΔS}}^{\text{0}}\text{is}\text{the}\text{standard}\text{entropy}\text{change}\end{array}$

(c)

Interpretation Introduction

Interpretation:

The variation of $\Delta S^0$ if $\Delta H^0=0kcalmo{l}^{-1}$ should be determined.

Concept introduction:

Gibbs free energy change $\Delta G^0$: The difference between the free energy of the products and the free energy of reactants under standard conditions is called Gibbs free energy change.

Gibbs free energy change $\Delta G^0$ can be formulated in terms of enthalpy, entropy and temperature as,

$\begin{array}{l}{\text{ΔG}}^{\text{0}}\text{=}{\text{ΔH}}^{\text{0}}\text{-}{\text{TΔS}}^{\text{0}}\\ {\text{ΔH}}^{\text{0}}\text{is}\text{the}\text{standard}\text{enthalpy}\text{change}\\ {\text{ΔS}}^{\text{0}}\text{is}\text{the}\text{standard}\text{entropy}\text{change}\end{array}$