Chapter 18, Problem 18.99QP

Interpretation Introduction

Interpretation:

The formation 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 formation constant: Free energy and equilibrium constant are related by the given equation.

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

Where,

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

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

${\text{K}}_{\text{f}}$ is the formation constant