   # It took 150. s for a current of 1.25 A to plate out 0.109 g of a metal from a solution containing its cations. Show that it is not possible for the cations to have a charge of 1+. ### 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 130AE
Textbook Problem
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## It took 150. s for a current of 1.25 A to plate out 0.109 g of a metal from a solution containing its cations. Show that it is not possible for the cations to have a charge of 1+.

Interpretation Introduction

Interpretation:

The reason behind the absence of +1 charge over the given metal for a given amount of metal that is deposited when a given amount of current is passed for a certain period of time is to be stated.

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 reason behind the absence of +1 charge over the given metal for a given amount of metal that is deposited when a given amount of current is passed for a certain period of time.

### Explanation of Solution

Given,

The amount of current passed is 1.25A .

The time period is 150.0s .

The amount of gas metal is 0.109g .

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

Where,

• Q is the charge carried in the cell.
• I is the current in amperes.
• t is the time for which current is passed through the cell.
• Z is the electrochemical equivalent.

Rearrange the equation to obtain the value of Z .

Z=WIt

Substitute the value of W , I and t in the above equation as,

Z=WIt=0.109g1.25A×150s=5.8×104g/C

The value of Z is given as,

Z=Molarmassn×96,485=E96,485Cmolee

Where,

• E is the equivalent weight

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