Chapter 19, Problem 19.124SP

Interpretation Introduction

Interpretation:

The equilibrium constant for the given reaction has to be calculated.

Concept Introduction:

The standard electrode potential of a cell${\text{(E}}^{°}{}_{\text{cell}})$ is the difference in electrode potential of the cathode and anode.

  ${\text{E}}^{\text{°}}{}_{\text{cell}}={\text{E}}^{\text{°}}{}_{\text{cathode}}-{\text{E}}^{\text{°}}{}_{\text{anode}}$

The relation between electrode potential and equilibrium constant: standard electrode potential and equilibrium constant are related by the given equation.

  ${\text{E}}^{°}{}_{\text{cell}}\text{=}\frac{\text{0}\text{.0592V}}{\text{n}}\text{logK}$

Where,

  ${\text{E}}^{°}{}_{\text{cell}}$ is the standard electrode potential

  $\text{n}$ is the number of electrons

  $\text{K}$ is the equilibrium constant