   # In the electrolysis of a solution containing Ni 2+ (aq), metallic Ni(s) deposits on the cathode. Using a current of 0.150 A for 12.2 minutes, what mass of nickel will form? ### 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 47PS
Textbook Problem
166 views

## In the electrolysis of a solution containing Ni2+(aq), metallic Ni(s) deposits on the cathode. Using a current of 0.150 A for 12.2 minutes, what mass of nickel will form?

Interpretation Introduction

Interpretation:

The mass of nickel during the electrolysis of solution which contains Ni2+(aq), metallic Ni(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 12.2 min.

Charge = Current(A) × time(s)Current = 0.150 Atime = 12.2min × 60.0sec. min-1

Substitute the values, we get charge of the cell.

Charge = (0.150 A) × (12.2 min)(60.0 sec.min-1)=109.8 C

Let’s calculate the moles electrons:

1mole = (109.8 C)(1 mol e-96500 C)=1

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