   Chapter 19, Problem 48PS

Chapter
Section
Textbook Problem

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

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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