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The reduction of aluminum ions occurs as: Al³+ (aq) + 3e → Al(s) After applying a certain amount of current through an electrolytic cell, 0.1328 g of aluminum is deposited at the electrode a. How many moles of aluminum metal has been deposited? www b.How many aluminum atoms have been deposited? (Use Avogadro's number). c. How many electrons were required for the reduction of this much aluminum?

The reduction of aluminum ions occurs as: Al³+ (aq) + 3e → Al(s) After applying a certain amount of current through an electrolytic cell, 0.1328 g of aluminum is deposited at the electrode a. How many moles of aluminum metal has been deposited? www b.How many aluminum atoms have been deposited? (Use Avogadro's number). c. How many electrons were required for the reduction of this much aluminum?

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.123QP: An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39...
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2. The reduction of aluminum ions occurs as: Al³+ (aq) + 3e → Al(s) After applying a certain amount of current through an electrolytic cell, 0.1328 g of aluminum is deposited at the electrode a. How many moles of aluminum metal has been deposited? b.How many aluminum atoms have been deposited? (Use Avogadro's number). c. How many electrons were required for the reduction of this much aluminum? d. If the electronic charge is 1.60 x 10-¹C, what is the total electrical charge used? e. If a constant current of 90 mA were applied, what was the time elapsed in seconds and in minutes?
Transcribed Image Text:2. The reduction of aluminum ions occurs as: Al³+ (aq) + 3e → Al(s) After applying a certain amount of current through an electrolytic cell, 0.1328 g of aluminum is deposited at the electrode a. How many moles of aluminum metal has been deposited? b.How many aluminum atoms have been deposited? (Use Avogadro's number). c. How many electrons were required for the reduction of this much aluminum? d. If the electronic charge is 1.60 x 10-¹C, what is the total electrical charge used? e. If a constant current of 90 mA were applied, what was the time elapsed in seconds and in minutes?
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