   # A factory wants to produce 1.00 × 10 3 kg barium from the electrolysis of molten barium chloride. What current must be applied for 4.00 h to accomplish this? ### 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 17, Problem 102E
Textbook Problem
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## A factory wants to produce 1.00 × 103 kg barium from the electrolysis of molten barium chloride. What current must be applied for 4.00 h to accomplish this?

Interpretation Introduction

Interpretation:

The amount of Barium produced from the electrolysis of molten Barium chloride is given. The amount of current that is to be supplied to accomplish the reaction 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,

W=ZQ=ZIt

The value of Z is given as,

Z=Molarmassn×96,485

To determine: The amount of current to be supplied to produce given amount of Barium from the electrolysis of molten Barium chloride.

### Explanation of Solution

Given information

The amount of Barium produced is 1.00×103kg .

The given time is 4.0h .

The conversion of kg to g is done as,

1kg=1000g

Therefore, the conversion of 1.00×103kg into g is,

1.00×103kg=1.00×103×1000g=106g

The conversion of h to sec is done as,

1h=3600sec

The conversion of 4h to sec is done as,

4h=4×3600sec=14400sec

The reaction showing electrolysis of molten Barium chloride is,

Ba2+(aq)+2Cl-(aq)+2e-Ba(s)+Cl2(g)+2e-

The value of Z is given as,

Z=Molarmassn×96,485=E96,485

Where,

• n is the number of electrons exchanged.
• E is the equivalent weight.
• Z is the electrochemical equivalent.

The reaction involves the transfer of 2 moles of electrons

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