Chapter 9, Problem 9.126SP

Interpretation Introduction

Interpretation:

The reactions (a) − (d) that are nonspontaneous at all temperature and the reactions (a) − (d) the have an equilibrium temperature should be determine.

Concept introduction:

The $\Delta \mathrm{G}$defines if the reaction is spontaneous or nonspontaneous in the following way,

If $\Delta \mathrm{G}$<0 the reaction is spontaneous.

If $\Delta \mathrm{G}$ =0 the reaction is in equilibrium.

If $\Delta \mathrm{G}$ >0 the reaction is nonspontaneous.

The free-energy change $\Delta \mathrm{G}$ can be defined of thefollowing way,

$\Delta \mathrm{G}=\Delta \text{H}-\text{TΔS}$

Where $\Delta \text{H}$ is the enthalpy change of the reaction, $\text{ΔS}$ is the entropy change of the reaction and T is the temperature.