Chapter 14, Problem 14.31P

Interpretation Introduction

Interpretation:

The net cell reaction and its equilibrium constant has to be calculated.

Concept introduction:

Nernst equation can be used to determine the cell potential at any instant, the difference from the standard state.

${\text{E = E}}^{\text{o }}\text{- }\frac{\text{0}\text{.05916}}{\text{n}}\text{log}\frac{{\left[\text{B}\right]}^{\text{b}}{\left[{\text{H}}^{\text{+}}\right]}^{\text{m}}}{{\left[\text{A}\right]}^{\text{a}}}$

Where:

$\text{E}$ = cell potential under nonstandard conditions

$\text{E}{}_{}^{\text{o}}$ = cell potential under standard conditions
n = number of moles of electrons exchanged in the electrochemical reaction

Finding $\text{K}$ from ${\text{E}}^{\text{o}}$

$\text{K}\text{=}\frac{{\text{10}}^{{\text{nE}}^{\text{o}}}}{\text{0}\text{.05916}}\text{at}{\text{25}}^{\text{o}}\text{C}$

Where $\text{K}$ is equilibrium constant