Chapter 21, Problem 21.182QP

Interpretation Introduction

Interpretation:

The standard electrode potential and standard free energy of the given reaction has to be calculated.  Also the spontaneity of the reaction has to be predicted.

Concept introduction:

Gibbs free energy: 

The largest amount of work which can be achieved through closed system.  This can be attained in reversible process.

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

If the ${\text{ΔG}}^{\text{o}}\text{<}\text{0}$, that is negative, the reaction is spontaneous.

If the ${\text{ΔG}}^{\text{o}}>\text{0}$, that is positive, the reaction is non-spontaneous.

If the ${\text{ΔG}}^{\text{o}}\text{=}\text{0}$, the reaction is equilibrium.