Chapter 6, Problem 6C.4P

(a)

Interpretation Introduction

Interpretation: The effect of the specified changes made to the given cell on the cell potential has to be stated.

Concept introduction: Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations.  The expression for Nernst equation is,

    $E_{\text{cell}}=E_{\text{cell}}^{\text{ο}}-\frac{RT}{vF}\ln Q$

Where,

• $E_{\text{cell}}$ is the electrode potential of the cell.
• $E_{\text{cell}}^{\text{ο}}$ is the standard electrode potential of the cell.
• $R$ is the gas constant.
• $T$ is the temperature.
• $v$ is the number of electrons.
• $F$ is the Faraday’s constant.
• $Q$ is the reaction quotient.

(b)

Interpretation Introduction

Interpretation: The effect of the specified changes made to the given cell on the cell potential has to be stated.

Concept introduction: Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations.  The expression for Nernst equation is,

    $E_{\text{cell}}=E_{\text{cell}}^{\text{ο}}-\frac{RT}{vF}\ln Q$

Where,

• $E_{\text{cell}}$ is the electrode potential of the cell.
• $E_{\text{cell}}^{\text{ο}}$ is the standard electrode potential of the cell.
• $R$ is the gas constant.
• $T$ is the temperature.
• $v$ is the number of electrons.
• $F$ is the Faraday’s constant.
• $Q$ is the reaction quotient.

(c)

Interpretation Introduction

Interpretation: The effect of the specified changes made to the given cell on the cell potential has to be stated.

Concept introduction: Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations.  The expression for Nernst equation is,

    $E_{\text{cell}}=E_{\text{cell}}^{\text{ο}}-\frac{RT}{vF}\ln Q$

Where,

• $E_{\text{cell}}$ is the electrode potential of the cell.
• $E_{\text{cell}}^{\text{ο}}$ is the standard electrode potential of the cell.
• $R$ is the gas constant.
• $T$ is the temperature.
• $v$ is the number of electrons.
• $F$ is the Faraday’s constant.
• $Q$ is the reaction quotient.

(d)

Interpretation Introduction

Interpretation: The effect of the specified changes made to the given cell on the cell potential has to be stated.

Concept introduction: Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations.  The expression for Nernst equation is,

    $E_{\text{cell}}=E_{\text{cell}}^{\text{ο}}-\frac{RT}{vF}\ln Q$

Where,

• $E_{\text{cell}}$ is the electrode potential of the cell.
• $E_{\text{cell}}^{\text{ο}}$ is the standard electrode potential of the cell.
• $R$ is the gas constant.
• $T$ is the temperature.
• $v$ is the number of electrons.
• $F$ is the Faraday’s constant.
• $Q$ is the reaction quotient.

(e)

Interpretation Introduction

Interpretation: The effect of the specified changes made to the given cell on the cell potential has to be stated.

Concept introduction: Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations.  The expression for Nernst equation is,

    $E_{\text{cell}}=E_{\text{cell}}^{\text{ο}}-\frac{RT}{vF}\ln Q$

Where,

• $E_{\text{cell}}$ is the electrode potential of the cell.
• $E_{\text{cell}}^{\text{ο}}$ is the standard electrode potential of the cell.
• $R$ is the gas constant.
• $T$ is the temperature.
• $v$ is the number of electrons.
• $F$ is the Faraday’s constant.
• $Q$ is the reaction quotient.

(f)

Interpretation Introduction

Interpretation: The effect of the specified changes made to the given cell on the cell potential has to be stated.

Concept introduction: Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations.  The expression for Nernst equation is,

    $E_{\text{cell}}=E_{\text{cell}}^{\text{ο}}-\frac{RT}{vF}\ln Q$

Where,

• $E_{\text{cell}}$ is the electrode potential of the cell.
• $E_{\text{cell}}^{\text{ο}}$ is the standard electrode potential of the cell.
• $R$ is the gas constant.
• $T$ is the temperature.
• $v$ is the number of electrons.
• $F$ is the Faraday’s constant.
• $Q$ is the reaction quotient.