   Chapter 19, Problem 106IL

Chapter
Section
Textbook Problem

An old method of measuring the current flowing in a circuit was to use a “silver coulometer.” The current passed first through a solution of Ag+(aq) and then into another solution containing an electroactive species. The amount of silver metal deposited at the cathode was weighed. From the mass of silver, the number of atoms of silver was calculated. Since the reduction of a silver ion requires one electron, this value equaled the number of electrons passing through the circuit. If the time was noted, the average current could he calculated. If, in such an experiment, 0.052 g of Ag is deposited during 450 s, what was the current flowing in the circuit?

Interpretation Introduction

Interpretation:

The current flowing in the electrolytic cell in 450s.has to be determined if 0.052g of Ag is deposited.

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 charge with change in time is called current.

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 write the half reaction.

Ag+(aq) + e- Ag(s)

Let’s calculate the number of moles of electrons:

Mole of e-= (0.052 g)(1 molAg)(1 mol e

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