Chapter 19, Problem 108FP

Interpretation Introduction

(a)

Interpretation:

The given equation needs to be derived.

${\Delta }_r{G}^o={\Delta }_r{G}^{*}-\Delta v_{\text{gas}}\ln \left(\frac{P^o}{P^{\ast }}\right)$

Concept introduction:

The relation between ${\Delta }_r{G}^o$ and ${\Delta }_r{G}^{*}$ is represented as follows:

${\Delta }_r{G}^o={\Delta }_r{G}^{*}-\Delta v_{\text{gas}}\ln \left(\frac{P^o}{P^{\ast }}\right)$

Here, ${\Delta }_r{G}^o$ and ${\Delta }_r{G}^{*}$ Gibbs free energy of reaction $P^o=1\text{ bar}$ and $P^{\ast }=1\text{ atm}$ respectively and $\Delta v_{\text{gas}}$ is change in number of gases.

Interpretation Introduction

(b)

Interpretation:

The following equation needs to be derived.

$E^o{}_{\text{cell}}=E^{\ast }{}_{\text{cell}}+3.382\times {10}^{-4}\text{V}\left(\Delta v_{\text{gas}}/z\right)$

Concept introduction:

The relation between $\Delta G$ and $E_{\text{cell}}$ is represented as follows:

$\Delta G=-zF{E}_{\text{cell}}$

Here, z is number of electrons transferred in the reaction, F is Faraday’s constant and $E_{\text{cell}}$ is electrode potential of the cell.

Interpretation Introduction

(c)

Interpretation:

The difference between $E^o{}_{\text{cell}}$ and $E^{\ast }{}_{\text{cell}}$ needs to be determined.

Concept introduction:

The relation between $\Delta G$ and $E_{\text{cell}}$ is represented as follows:

$\Delta G=-zF{E}_{\text{cell}}$

Here, z is number of electrons transferred in the reaction, F is Faraday’s constant and $E_{\text{cell}}$ is electrode potential of the cell.

Interpretation Introduction

(d)

Interpretation:

The value for $E^o{}_{\text{cell}}$ is 0.956 V for the overall reaction. The corresponding value of $E^{\ast }{}_{\text{cell}}$ needs to be determined.

Concept introduction:

The relation between $\Delta G$ and $E_{\text{cell}}$ is represented as follows:

$\Delta G=-zF{E}_{\text{cell}}$

Here, z is number of electrons transferred in the reaction, F is Faraday’s constant and $E_{\text{cell}}$ is electrode potential of the cell.