Chapter 21, Problem 21.54P

(a)

Interpretation Introduction

Interpretation:

The response of $E_{cell}$ when cell temperature is decreased has to be identified.

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The Nernst equation depicts the relationship between $E_{cell}$ and ${\text{E}}^{\text{o}}{}_{\text{cell}}$ as follows,

$\begin{array}{l}{\text{E}}_{\text{cell}}{\text{ = E}}^{\text{o}}{}_{\text{cell}}-\frac{RT}{nF}\log Q\\ \\ \boxed{\begin{array}{c}where,{\text{E}}_{\text{cell}}=cellpotential\\ {\text{E}}^{\text{o}}{}_{\text{cell}}=\text{Standard}cellpotential\\ n=No.ofelectrons\\ Q=\text{Reaction}Quotient\\ R=G\text{as}\text{constant}\\ \text{T}\text{=}\text{Temperature}\end{array}}\end{array}$

(b)

Interpretation Introduction

Interpretation:

The response of $E_{cell}$ when active ion concentration in anode compartment is increased has to be identified.

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The Nernst equation depicts the relationship between $E_{cell}$ and ${\text{E}}^{\text{o}}{}_{\text{cell}}$ as follows,

$\begin{array}{l}{\text{E}}_{\text{cell}}{\text{ = E}}^{\text{o}}{}_{\text{cell}}-\frac{RT}{nF}\log Q\\ \\ \boxed{\begin{array}{c}where,{\text{E}}_{\text{cell}}=cellpotential\\ {\text{E}}^{\text{o}}{}_{\text{cell}}=\text{Standard}cellpotential\\ n=No.ofelectrons\\ Q=\text{Reaction}Quotient\\ R=G\text{as}\text{constant}\\ \text{T}\text{=}\text{Temperature}\end{array}}\end{array}$

(c)

Interpretation Introduction

Interpretation:

The response of $E_{cell}$ when active ion concentration in cathode compartment is increased has to be identified.

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The Nernst equation depicts the relationship between $E_{cell}$ and ${\text{E}}^{\text{o}}{}_{\text{cell}}$ as follows,

$\begin{array}{l}{\text{E}}_{\text{cell}}{\text{ = E}}^{\text{o}}{}_{\text{cell}}-\frac{RT}{nF}\log Q\\ \\ \boxed{\begin{array}{c}where,{\text{E}}_{\text{cell}}=cellpotential\\ {\text{E}}^{\text{o}}{}_{\text{cell}}=\text{Standard}cellpotential\\ n=No.ofelectrons\\ Q=\text{Reaction}Quotient\\ R=G\text{as}\text{constant}\\ \text{T}\text{=}\text{Temperature}\end{array}}\end{array}$

(d)

Interpretation Introduction

Interpretation:

The response of $E_{cell}$ when pressure of gaseous reactant in cathode compartment is increased has to be identified.

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The Nernst equation depicts the relationship between $E_{cell}$ and ${\text{E}}^{\text{o}}{}_{\text{cell}}$ as follows,

$\begin{array}{l}{\text{E}}_{\text{cell}}{\text{ = E}}^{\text{o}}{}_{\text{cell}}-\frac{RT}{nF}\log Q\\ \\ \boxed{\begin{array}{c}where,{\text{E}}_{\text{cell}}=cellpotential\\ {\text{E}}^{\text{o}}{}_{\text{cell}}=\text{Standard}cellpotential\\ n=No.ofelectrons\\ Q=\text{Reaction}Quotient\\ R=G\text{as}\text{constant}\\ \text{T}\text{=}\text{Temperature}\end{array}}\end{array}$