Chapter 22, Problem 22.45P

(a)

Interpretation Introduction

Interpretation:

The minimum energy required to form one mole of hydrogen gas has to be calculated.

Concept Introduction:

The relationship between standard cell potential and Gibb’s free energy is given by

    $\begin{array}{l}{\text{ΔG}}^{\text{o}}\text{=}{\text{-nFE}}^{\text{o}}\\ \\ {\text{ΔG}}^{\text{o}}\text{is}\text{change}\text{in}\text{Gibbs}\text{free}\text{energy}\text{at}\text{standard}\text{conditions}\\ \\ \text{n}\text{is}\text{number}\text{of}\text{moles}\text{of}\text{electrons}\\ \\ \text{F = Faraday constant (96485 C/mol)}\\ \\ \text{E° = standard cell potential}\end{array}$

(b)

Interpretation Introduction

Interpretation:

The energy efficiency of cell operation has to be calculated.

Concept introduction:

The energy efficiency of a cell is calculated as,

    $\text{Efficiency = }\left[\frac{\text{(useful work done)}}{\text{(energy input)}}\right]\text{ x 100\%}$

(c)

Interpretation Introduction

Interpretation:

The cost of producing $\text{500mol}$ of hydrogen has to be calculated.