   # Assume the specifications of a Ni-Cd voltaic cell include delivery of 0.25 A of current for 1.00 hour. What is the minimum mass of the cadmium that must be used to make the anode in this cell? ### 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 52PS
Textbook Problem
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## Assume the specifications of a Ni-Cd voltaic cell include delivery of 0.25 A of current for 1.00 hour. What is the minimum mass of the cadmium that must be used to make the anode in this cell?

Interpretation Introduction

Interpretation:

The minimum mass of cadmium at anode has to be determined if the Ni-Cd voltaic cell include delivery of 0.25 A current for 1.00 hr.

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

The half cell reaction of the Cadmium is as follows.

Cd2+(aq) + 2e-  Cd(s)

Let’s calculate the charge in the cell in 1.00 h.

Charge =Current×timeCurrent = 0.25Atime =1.00h

Substitute the values and calculate the charge of the cell:

= 0.25A × 1

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