Chapter 19.4, Problem 1Q

(a)

Interpretation Introduction

Interpretation:

The energy released for each mole of lithium oxidised during the discharge of the battery has to be determined if the battery produces a voltage of $\text{3}\text{.6}\text{V}$.

Concept introduction:

In voltaic cell, the maximum cell potential is directly related to the free energy difference between the reactants and products in the cell.

$\begin{array}{c}{\text{ΔG}}^{\text{0}}{\text{= -nFE}}^{\text{0}}\\ \text{n = Number of moles transferred per mole of reactant and products}\\ \text{F = Faradayconstant=96485C/mol}\\ {\text{ E}}^{\text{0}}\text{= Volts = Work(J)/Charge(C)}\end{array}$

The relation between standard cell potential and equilibrium constant is as follows.

$\text{lnK = }\frac{{\text{nE}}^{\text{0}}}{\text{0}\text{.0257}}\text{ at 298K}$

(b)

Interpretation Introduction

Interpretation:

The energy released per kilogram of lithium has to be determined.

Concept introduction:

In voltaic cell, the maximum cell potential is directly related to the free energy difference between the reactants and products in the cell.

$\begin{array}{c}{\text{ΔG}}^{\text{0}}{\text{= -nFE}}^{\text{0}}\\ \text{n = Number of moles transferred per mole of reactant and products}\\ \text{F = Faradayconstant=96485C/mol}\\ {\text{ E}}^{\text{0}}\text{= Volts = Work(J)/Charge(C)}\end{array}$

The relation between standard cell potential and equilibrium constant is as follows.

$\text{lnK = }\frac{{\text{nE}}^{\text{0}}}{\text{0}\text{.0257}}\text{ at 298K}$