Chapter 19, Problem 21E

Interpretation Introduction

(a)

Interpretation:

The standard cell potential needs to be determined, whether the reaction is spontaneousor not needs to be explained.

${\text{H}}_{\text{2}}\left(g\right)+{\text{F}}_{\text{2}}\left(g\right)\to 2{\text{H}}^{+}\left(aq\right)+{\text{2F}}^{-}\left(aq\right)$

Concept introduction:

There should be positive $E{°}_{\text{cell}}$ value in order to accomplish any reaction for the given direction. This is because for every spontaneous reaction, the value of $\Delta G^o$ should be negative. The relation between $\Delta G^o$ and $E{°}_{\text{cell}}$ is represented as follows:

$\Delta G^o=-nFE{°}_{\text{cell}}$

For positive value of $E{°}_{\text{cell}}$, the value of $\Delta G^o$ will be negative.

The $E{°}_{\text{cell}}$ value for a redox reaction is given by following equation.

$E{°}_{\text{cell}}=E{°}_{\text{Reduction}}-E{°}_{\text{Oxidation}}$

Interpretation Introduction

(b)

Interpretation:

The standard cell potential needs to be determined, whether the reaction is spontaneousor not needs to be explained.

$\text{Cu}\left(s\right)+{\text{Ba}}^{2+}\left(aq\right)\to {\text{Cu}}^{2+}\left(aq\right)+\text{Ba}\left(s\right)$

Concept introduction:

There should be positive $E{°}_{\text{cell}}$ value in order to accomplish any reaction for the given direction. This is because for every spontaneous reaction, the value of $\Delta G^o$ should be negative. The relation between $\Delta G^o$ and $E{°}_{\text{cell}}$ is represented as follows:

$\Delta G^o=-nFE{°}_{\text{cell}}$

For positive value of $E{°}_{\text{cell}}$, the value of $\Delta G^o$ will be negative.

The $E{°}_{\text{cell}}$ value for a redox reaction is given by following equation.

$E{°}_{\text{cell}}=E{°}_{\text{Reduction}}-E{°}_{\text{Oxidation}}$

Interpretation Introduction

(c)

Interpretation:

The standard cell potential needs to be determined, whether the reaction is spontaneousor not needs to be explained.

${\text{3Fe}}^{2+}\left(aq\right)\to \text{Fe}\left(s\right)+2{\text{Fe}}^{3+}\left(aq\right)$

Concept introduction:

There should be positive $E{°}_{\text{cell}}$ value in order to accomplish any reaction for the given direction. This is because for every spontaneous reaction, the value of $\Delta G^o$ should be negative. The relation between $\Delta G^o$ and $E{°}_{\text{cell}}$ is represented as follows:

$\Delta G^o=-nFE{°}_{\text{cell}}$

For positive value of $E{°}_{\text{cell}}$, the value of $\Delta G^o$ will be negative.

The $E{°}_{\text{cell}}$ value for a redox reaction is given by following equation.

$E{°}_{\text{cell}}=E{°}_{\text{Reduction}}-E{°}_{\text{Oxidation}}$

Interpretation Introduction

(d)

Interpretation:

The standard cell potential needs to be determined, whether the reaction is spontaneousor not needs to be explained.

$\text{Hg}\left(l\right)+{\text{HgCl}}_{\text{2}}\left(aq\right)\to {\text{Hg}}_2{\text{Cl}}_{\text{2}}\left(s\right)$

Concept introduction:

There should be positive $E{°}_{\text{cell}}$ value in order to accomplish any reaction for the given direction. This is because for every spontaneous reaction, the value of $\Delta G^o$ should be negative. The relation between $\Delta G^o$ and $E{°}_{\text{cell}}$ is represented as follows:

$\Delta G^o=-nFE{°}_{\text{cell}}$

For positive value of $E{°}_{\text{cell}}$, the value of $\Delta G^o$ will be negative.

The $E{°}_{\text{cell}}$ value for a redox reaction is given by following equation.

$E{°}_{\text{cell}}=E{°}_{\text{Reduction}}-E{°}_{\text{Oxidation}}$