   Chapter 19, Problem 50PS

Chapter
Section
Textbook Problem

Electrolysis of a solution of Zn(NO3)2(aq) to give zinc metal is carried out using a current of 2.12 A. How long should electrolysis continue in order to prepare 2.5 g of zinc?

Interpretation Introduction

Interpretation:

The time required to give Zinc metal by the electrolysis of a solution of Zn(NO3)2(aq) has to be determined using a current of 2.12 A.

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

The half cell reaction of the copper is as follows.

Zn2+(aq) + 2e-  Zn(s)

The given mass of Zinc = 2.5 g.

Let’s calculate the moles electrons:

1mol e = (2.5 g Zn)(1 mol Zn65.4 g Zn)(2 mol e-1 mol Zn)= 7.645×10-2 mol e-

Let’s calculate the charge in the cell:

Charge (C) = (7

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