Chapter 19, Problem 19.108SP

Interpretation Introduction

Interpretation:

From the relation between ${\text{E}}^{\circ }$, $\Delta G^{\circ }$ and K, this is to be shown that the value of $\Delta G^{\circ }$ is negative and $K>1$ for the reaction with a positive ${\text{E}}^{\circ }$ value.

Concept introduction:

The substances that have a higher reduction potential will undergo reduction at the cathode while the substances that have a lower reduction potential will undergo oxidation at the anode.

The expression to calculate the equilibrium constant is shown below:

$\Delta G_{\text{cell}}^o=-\text{RT}\ln \text{K}$

Here, R is Universal gas constant, T is temperature and K is equilibrium constant.

The expression to calculate the standard Gibbs free energy of the cell is shown below:

$\Delta G_{\text{cell}}^o=-{\text{nFE}}_{\text{cell}}^o$

Here, n is the number of electrons transferred, F is Faraday’s constant and ${\text{E}}_{\text{cell}}^o$ is standard electrode potential of the cell.