Chapter 17, Problem 110E

(a)

Interpretation Introduction

Interpretation:

The reactions that take place at the cathode and the anode when molten $\text{KF}$, ${\text{CuCl}}_2$ and ${\text{MgI}}_2$ are electrolyzed.

Concept introduction:

The non-spontaneous reaction takes place in an electrolytic cell in which there occurs conversion of electrical energy into chemical energy and this is used for the electrolysis of a metal. The electrolytic cell involves a cathode and an anode, both dipped into an electrolytic solution having both the positive and negative ions.

To determine: The reactions that take place at the cathode and the anode when molten $\text{KF}$ is electrolyzed.

The reaction taking place at cathode is,

${\text{K}}^{+}+{\text{e}}^{-}\to \text{K}$

The reaction taking place at anode is,

${\text{F}}^{-}\to \frac{1}{2}{\text{F}}_{\text{2}}{\text{+e}}^{-}$

(b)

Interpretation Introduction

Interpretation:

The reactions that take place at the cathode and the anode when molten $\text{KF}$, ${\text{CuCl}}_2$ and ${\text{MgI}}_2$ are electrolyzed.

Concept introduction:

The non-spontaneous reaction takes place in an electrolytic cell in which there occurs conversion of electrical energy into chemical energy and this is used for the electrolysis of a metal. The electrolytic cell involves a cathode and an anode, both dipped into an electrolytic solution having both the positive and negative ions.

To determine: The reactions that take place at the cathode and the anode when molten ${\text{CuCl}}_2$ is electrolyzed.

The reaction taking place at cathode is,

${\text{Cu}}^{2+}+2{\text{e}}^{-}\to \text{Cu}$

The reaction taking place at anode is,

$2{\text{Cl}}^{-}\to {\text{Cl}}_{\text{2}}\text{+}2{\text{e}}^{-}$

(c)

Interpretation Introduction

Interpretation:

The reactions that take place at the cathode and the anode when molten $\text{KF}$, ${\text{CuCl}}_2$ and ${\text{MgI}}_2$ are electrolyzed.

Concept introduction:

The non-spontaneous reaction takes place in an electrolytic cell in which there occurs conversion of electrical energy into chemical energy and this is used for the electrolysis of a metal. The electrolytic cell involves a cathode and an anode, both dipped into an electrolytic solution having both the positive and negative ions.

To determine: The reactions that take place at the cathode and the anode when molten ${\text{MgI}}_2$ is electrolyzed.

The reaction taking place at cathode is,

${\text{Mg}}^{2+}+2{\text{e}}^{-}\to \text{Mg}$

The reaction taking place at anode is,

$2{\text{I}}^{-}\to {\text{I}}_{\text{2}}\text{+}2{\text{e}}^{-}$