Chapter 21.4, Problem 21.6BFP

Interpretation Introduction

Interpretation: The value of K and $E_{\text{cell}}^{\text{o}}$ for the given reaction needs to be calculated at $25{}^{\text{o}}\text{C}$ .

Concept Introduction: The relation between change in standard Gibbs free energy and equilibrium constant of a reaction is as follows:

  $\Delta G^o=-RT\ln K$

Here, R is the universal gas constant and T is temperature.

Similarly, the relationship between change in standard Gibbs free energy and electrode potential of the cell is as follows:

  $\Delta G^o=-nF{E}_{cell}^o$

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