Calculate the number of grams of aluminum produced in 1.04 hour by the electrolysis of molten AICI3 if the electrical current is 18.097 A. Recall that: C = A*s Faraday's constant, F, is 96,485 C/mole of electrons. Al3+ + 3 e→ Al

Calculate the number of grams of aluminum produced in 1.04 hour by the electrolysis of molten AICI3 if the electrical current is 18.097 A. Recall that: C = A*s Faraday's constant, F, is 96,485 C/mole of electrons. Al3+ + 3 e→ Al

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 35QRT

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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

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Calculate the number of grams of aluminum produced in 1.04 hour by the electrolysis of molten
AICI3 if the electrical current is 18.097 A.
Recall that:
C = A*s
Faraday's constant, F, is 96,485 C/mole of electrons.
Al3+ + 3 e → Al

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