Chapter 21, Problem 91GQ

Interpretation Introduction

Interpretation:

To calculate the reaction is reactant or product favored at equliribrium at $\text{298 K}$ and the reaction is more or less product favored at higher temperature.

Concept introduction:

The $\Delta S^{\circ }\left(\text{system}\right)$ can be calculated by the following expression,

$\Delta S^{\circ }\left(\text{system}\right)={\text{Δ}}_{\text{r}}{S}^{\text{°}}=\sum n{S}^{\text{°}}\left(\text{products}\right)-\sum n{S}^{\text{°}}\left(\text{reactants}\right)$

Enthalpy of formation of the reaction can be calculated by following expression,

${\text{Δ}}_{\text{r}}{H}^{\text{°}}=\sum n{\Delta }_f{H}^{\text{°}}\left(\text{products}\right)-\sum n{\Delta }_f{H}^{\text{°}}\left(\text{reactants}\right)$

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by $\Delta G^{\circ }$. It is related to entropy and entropy by the following expression,

$\Delta G^{\circ }=\Delta H^{\circ }-T\Delta S^{\circ }$

Here, ${\Delta }_{\text{r}}{H}^{\circ }$ is the enthalpy change for the reaction.

If the value of ${\Delta }_{\text{r}}{G}^{\circ }$ is negative the reaction is product favored at equilibrium at $\text{298 K}$.