   # How long will it take to produce 1.00 × 10 3 kg of magnesium metal by the electrolysis of molten magnesium chloride using a current of 5.00 × 10 4 A? ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 19, Problem 22E
Textbook Problem
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## How long will it take to produce 1.00 × 103 kg of magnesium metal by the electrolysis of molten magnesium chloride using a current of 5.00 × 104 A?

Interpretation Introduction

Interpretation: The current required for the electrolysis of BaCl2 and the mass of magnesium produced is given. The time of the electrolysis for the production of magnesium is to be calculated.

Concept introduction: The process of decomposition of compounds by passing electricity through a solution is known as electrolysis.

To determine: The time for the production of magnesium during electrolysis.

### Explanation of Solution

Explanation

The reaction that takes place at cathode is,

Mg2+(aq)+2eMg(s)

The atomic mass of magnesium is 24.305g .

Formula

The electrochemical equivalence of electrolysis process is calculated as,

Z=AtomicmassofproductElectronsexchanged×96500C

Where,

• Z is the electrochemical equivalence.

Substitute the values of the atomic mass of magnesium and number of electrons exchanged in the above equation.

Z=AtomicmassofproductElectronsexchanged×96500C=24.305g2×96500C=1.26×104g/C_

The required time is 43.8h_ .

Given

Current passed during electrolysis is 5.00×104A .

Mass of magnesium produced is 1.00×103kg .

The value of electrochemical equivalence is 1.26×104g/C .

The conversion of kilogram (kg) into gram (g) is done as,

1kg=103g

Hence,

The conversion of 1.00×103kg into gram is,

1.00×103kg=(1

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