   # In the electrolysis of a solution containing Ag + (aq), metallic Ag(s) deposits on the cathode. Using a current of 1.12 A for 2.40 hours, what mass of silver forms? ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 19, Problem 48PS
Textbook Problem
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## In the electrolysis of a solution containing Ag+(aq), metallic Ag(s) deposits on the cathode. Using a current of 1.12 A for 2.40 hours, what mass of silver forms?

Interpretation Introduction

Interpretation:

The mass of silver formed during the electrolysis of solution which contains Ag+(aq), metallic Ag(s) deposits on the cathode has to be determined.

Concept introduction:

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.

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 of Solution

Let’s calculate the charge passing through the cell in 2.40 hours.

Charge = Current(A) × time(s)Current = 1.12 Atime = 2.40 h ×60 min h1 × 60.0sec. min-1

Substitute the values, we get charge of the cell.

Charge = (1.12 A) ×(2.40 h)×(60 min h1)× (60.0 sec.min-1)= 9.677×103 C

Let’s calculate the moles electrons:

1mole = (9

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