Chapter 19, Problem 19.120QP

Interpretation Introduction

Interpretation:

The standard reduction potential of fluorine has to be calculated.

Concept Introduction:

Standard reduction potential is the measure of the tendency of a species to undergo reduction.  It is measured in terms of volts.  The substance which is having high positive value will easily undergo reduction.

Free energy (Gibbs free energy) is the term that is used to explain the total energy content in a thermodynamic system that can be converted into work.  The free energy is represented by the letter $\text{G}$.  All spontaneous process is associated with the decrease of free energy in the system.  The standard free energy change ${\text{(ΔG}}^{\text{°}}{}_{\text{rxn}})$ is the difference in free energy of the reactants and products in their standard state.

${\text{ΔG}}^{\text{°}}{}_{\text{rxn}}\text{=}\sum {\text{nΔG}}_{\text{f}}{}^{\text{°}}\text{(Products)-}\sum {\text{mΔG}}_{\text{f}}{}^{\text{°}}\text{(Reactants)}$

Where, n is the number of moles

The standard electrode potential of a cell${\text{(E}}^{°}{}_{\text{cell}})$ is the difference in electrode potential of the cathode and anode.

${\text{E}}^{\text{°}}{}_{\text{cell}}={\text{E}}^{\text{°}}{}_{\text{cathode}}-{\text{E}}^{\text{°}}{}_{\text{anode}}$

The relation between Gibbs free energy and cell potential: The amount of energy in a system that can be converted into useful energy is defined as free energy in thermodynamics. 

Free energy and the cell potential is related by the given equation.

$\text{ΔG=-nFE}$

Where,

$\text{ΔG}$ is the change in free energy

$\text{n}$ is the number of electrons transferred

$\text{F}$ is the Faraday constant $\text{(F}={\text{96500Cmol}}^{\text{-1}})$

$\text{E}$ is the cell potential