Chapter 19, Problem 51PS

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

A voltaic cell can be built using the reaction between Al metal and O2 from the air. If the Al anode of this cell consists of 84 g of aluminum, how many hours can the cell produce 1.0 A of electricity, assuming an unlimited supply of O2?

Interpretation Introduction

Interpretation:

To determine the time required when a voltaic cell can be built using the reaction between Al metal and O2 from the air. The Al anode of this cell consists of 84 g of aluminium can the cell produce 1.0 A of electricity assuming an unlimited supply O2.

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 Aluminium is as follows.

Al3+(aq)Â +Â 3e-Â â†’Â Al(s)

The given mass of aluminium is 84g.

Letâ€™s calculate the moles electrons:

1molÂ eâˆ’Â =Â (84Â gÂ Al)(1Â molÂ Al27Â gÂ Al)(3Â molÂ e-1Â molÂ Al)=Â 9.3Â molÂ e-

Letâ€™s calculate the charge in the cell:

ChargeÂ (C)Â =Â (9.3Â molÂ e-)(96500Â C1Â molÂ e-)=8

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