Chapter 17, Problem 17.64SP

(a)

Interpretation Introduction

Interpretation:

The standard cell potential and the standard free-energy for the given reaction has to be calculated.

Concept Introduction:

Standard cell potential:

The standard cell potential is the measure of individual potential of reversible electrode at standard state.  The conditions that makes cell potential to qualify as standard cell potential is when all the reactants and the product are in standard state that is solutes at $\text{1}\text{M}$ concentrations, partial pressure of gases at $\text{1}\text{atm,}$ solids and liquids in pure state, all at $\text{25°C}\text{.}$

Standard free-energy:

The standard cell potential related to the free-energy is given by the equation,

$\text{ΔG°}\text{=}\text{-nFE°}$

Where,

$\begin{array}{l}\text{n}\text{=}\text{number}\text{of}\text{moles}\text{of}\text{electrons}\text{transferred}\\ \text{F}\text{=}\text{Faraday}\text{constant}\text{(96,500}\text{C/mol}{\text{e}}^{\text{-}}\text{)}\\ \text{E°}\text{=}\text{Standard cell potential}\\ \text{ΔG°}\text{=}\text{Change in free-energy}\end{array}$

(b)

Interpretation Introduction

Interpretation:

The standard cell potential and the standard free-energy for the given reaction has to be calculated.

Concept Introduction:

Standard cell potential:

The standard cell potential is the measure of individual potential of reversible electrode at standard state.  The conditions that makes cell potential to qualify as standard cell potential is when all the reactants and the product are in standard state that is solutes at $\text{1}\text{M}$ concentrations, partial pressure of gases at $\text{1}\text{atm,}$ solids and liquids in pure state, all at $\text{25°C}\text{.}$

Standard free-energy:

The standard cell potential related to the free-energy is given by the equation,

$\text{ΔG°}\text{=}\text{-nFE°}$

Where,

$\begin{array}{l}\text{n}\text{=}\text{number}\text{of}\text{moles}\text{of}\text{electrons}\text{transferred}\\ \text{F}\text{=}\text{Faraday}\text{constant}\text{(96,500}\text{C/mol}{\text{e}}^{\text{-}}\text{)}\\ \text{E°}\text{=}\text{Standard cell potential}\\ \text{ΔG°}\text{=}\text{Change in free-energy}\end{array}$

(c)

Interpretation Introduction

Interpretation:

The standard cell potential and the standard free-energy for the given reaction has to be calculated.

Concept Introduction:

Standard cell potential:

The standard cell potential is the measure of individual potential of reversible electrode at standard state.  The conditions that makes cell potential to qualify as standard cell potential is when all the reactants and the product are in standard state that is solutes at $\text{1}\text{M}$ concentrations, partial pressure of gases at $\text{1}\text{atm,}$ solids and liquids in pure state, all at $\text{25°C}\text{.}$

Standard free-energy:

The standard cell potential related to the free-energy is given by the equation,

$\text{ΔG°}\text{=}\text{-nFE°}$

Where,

$\begin{array}{l}\text{n}\text{=}\text{number}\text{of}\text{moles}\text{of}\text{electrons}\text{transferred}\\ \text{F}\text{=}\text{Faraday}\text{constant}\text{(96,500}\text{C/mol}{\text{e}}^{\text{-}}\text{)}\\ \text{E°}\text{=}\text{Standard cell potential}\\ \text{ΔG°}\text{=}\text{Change in free-energy}\end{array}$