Chapter 14, Problem 14.22P

Interpretation Introduction

Interpretation:

${\text{E°}}_{{\text{Ag}}^{\text{+}}|\text{Ag}}$ has to be calculated using the measured cell voltage and activity coefficients.

Concept Introduction:

Nernst Equation:

For Half-reaction,

${\text{aA+ne}}^{\text{-}}\stackrel{}{\rightleftharpoons }\text{bB}$

The Nernst equation results in the half-cell potential E as,

$\text{E=E°-}\frac{\text{RT}}{\text{nF}}\text{ln}\frac{{\text{A}}_{\text{B}}{}^{\text{b}}}{{\text{A}}_{\text{A}}{}^{\text{a}}}$

Here,

$\text{E°}$ = standard reduction potential ( ${\text{A}}_{\text{A}}{\text{=A}}_{\text{B}}\text{=1}$ )

$\text{R}$ = gas constant $\left(\text{8}\text{.314}\text{J/}\left(\text{K}\text{.mol}\right)\right)\text{=8}\text{.314}\left(\left(\text{V}\text{.C}\right)\text{/}\left(\text{K}\text{.mol}\right)\right)$

T=Temperature (in K)

n=number of electrons in half-reaction

F=Faraday constant ( $\text{9}{\text{.649×10}}^{\text{4}}\text{C/mol}$ )

A=Activity of species, i