   Chapter 19, Problem 67GQ

Chapter
Section
Textbook Problem

The reaction occurring in the cell in which Al2O3 and aluminum salts are electrolyzed is Al3+(aq) + 3 e− → Al(s). If the electrolysis cell operates at 5.0 V and 1.0 × 105 A, what mass of aluminum metal can be produced in a 24-hour day?

Interpretation Introduction

Introduction:

To determine the mass of aluminium metal can be produced in a 24-hour day, If the electrolysis cell operates at 5.0 V and 1.0×105.

Explantion:

Electrolysis:

It is a decomposition of ionic compounds by passing electricity through molten compounds or aqueous solutions of compounds.

Electricity used to produce chemical changes. The apparatus used for electrolysis is called an electrolytic cell.

Current:

Rate of the charge changing in time is defined as the current.

The formula is as follows.

Current (Amperes, A) = Electric charge (Coloumbs, C)time, t(seconds,s)

Simplify as follows.

Current = Electric charge time

To rearrange the above formula is as follows.

Charge = Current(A) × time(s)

Explanation

Let’s calculate the charge passing through the cell in 24 hrs.

Charge = Current(A) × time(s)Current = 1.0×105 Atime = 24h ×60 min × 60.0sec. min-1

Substitute the values, we get charge of the cell.

Charge = (1.0×105 A) ×24 h× (60 min)(60.0 sec.min-1)=8.64×109 C

Let’s calculate the moles electrons:

1mole = (8

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