An industrial electrolytic process for producing aluminum uses the reactions shown in the following equations. Anode(oxidation)C(s)+2O2−(aq)⟶CO2(g)+4e−Anode(oxidation)C(�)+2O2−(��)⟶CO2(�)+4e− Cathode(reduction)Al3+(aq)+3e−⟶Al(s)Cathode(reduction)Al3+(��)+3e−⟶Al(�) How long would it take to produce enough aluminum to make a case (24 cans) of aluminum soft drink cans if each can used 5.502 g of aluminum, a current* of 285 kA was employed, and the current efficiency was 93%?
An industrial electrolytic process for producing aluminum uses the reactions shown in the following equations. Anode(oxidation)C(s)+2O2−(aq)⟶CO2(g)+4e−Anode(oxidation)C(�)+2O2−(��)⟶CO2(�)+4e− Cathode(reduction)Al3+(aq)+3e−⟶Al(s)Cathode(reduction)Al3+(��)+3e−⟶Al(�) How long would it take to produce enough aluminum to make a case (24 cans) of aluminum soft drink cans if each can used 5.502 g of aluminum, a current* of 285 kA was employed, and the current efficiency was 93%?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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An industrial electrolytic process for producing aluminum uses the reactions shown in the following equations.
Anode(oxidation)C(s)+2O2−(aq)⟶CO2(g)+4e−Anode(oxidation)C(�)+2O2−(��)⟶CO2(�)+4e−
Cathode(reduction)Al3+(aq)+3e−⟶Al(s)Cathode(reduction)Al3+(��)+3e−⟶Al(�)
How long would it take to produce enough aluminum to make a case (24 cans) of aluminum soft drink cans if each can used 5.502 g of aluminum, a current* of 285 kA was employed, and the current efficiency was 93%?
*That is not a typo; the currents used in aluminum production are huge, which is why recycling aluminum is usually more economical than producing it from ore.
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