Chapter 17, Problem 96E

Interpretation Introduction

Interpretation:

The production of aluminum by the electrolysis of ${\text{Al}}_2{\text{O}}_3$ in molten salt is given. The mass of aluminum that can be produced in $2.00\text{h}$ is to be calculated.

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 charge generated in the cell is calculated as,

$Q=It$

When electricity is passed through an electrolytic cell, at that time the amount of the substance that is liberated at an electrode is given by,

$\begin{array}{c}W=ZQ\\ =ZIt\end{array}$

The value of $Z$ is given as,

$Z=\frac{\text{Atomic}\text{mass}}{n\times 96,485}$

The mass of metal is calculated by multiplying the moles of metal with its atomic molar mass. This gives the mass of the metal to be plated out in the electrolytic cell.

To determine: The mass of aluminum that can be produced in $2.00\text{h}$ by the electrolysis of ${\text{Al}}_2{\text{O}}_3$ in molten salt.