Chapter 18, Problem 113AP

Interpretation Introduction

Interpretation:

The $\Delta G^{\circ }$

for the ionization of the acids, the dominant term in determining the value of $\Delta G^{\circ }$, the process that contributes to $\Delta H^{\circ }$

and the term $T\text{Δ}{S}^{\circ }$

is more negative for ${\text{CH}}_{\text{3}}\text{COOH}$, are to be explained.

Concept introduction:

The standard free energy change of the reaction is related to the equilibrium constant according to the given equation as follows:

$\Delta G^{\circ }\text{=}-\text{R}T\ln K$

Here, $\Delta G^{\circ }$

is the change in standard Gibbs free energy, $\text{R}$ is the universal gas constant, $T$

is the absolute temperature, and $K$

is the equilibrium constant.

The reaction is spontaneous if $\Delta G^{\circ }$

is negative.