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

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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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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