Explanation The half-reaction of the production of aluminum in the electrolysis is A l + 3 ( a q ) + 3 e − → A l ( s ) ss In this reaction, 1 mol of aluminum uses 3 moles of electrons. However, in the given problem, we have The magnitude of the current = 25 A Time taken to produce Al = 1 hour Thus, the mass of the Al produced is = 1 h o u r × 60 min 1 h o u r × 60 sec 1 min ×

Mastering Chemistry with Pearson eText -- Standalone Access Card -- for Chemistry: A Molecular Approach (4th Edition)

4th Edition

ISBN: 9780134162485

Author: Nivaldo J. Tro

Publisher: PEARSON

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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 electroly…

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Chapter 19, Problem 102E

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Interpretation: The mass of aluminum metal is to be calculated that can be produced by a current of 25 A per hour in the electrolysis of a molten aluminum salt.

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Chapter 19, Problem 101E

Chapter 19, Problem 103E

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Mastering Chemistry with Pearson eText -- Standalone Access Card -- for Chemistry: A Molecular Approach (4th Edition)

Ch. 19 - Prob. 1SAQ Ch. 19 - Q2. Which statement is true for voltaic cells? a)...Ch. 19 - Prob. 3SAQ Ch. 19 - Prob. 4SAQ Ch. 19 - Prob. 5SAQ Ch. 19 - Prob. 6SAQ Ch. 19 - Prob. 7SAQ Ch. 19 - Prob. 8SAQ Ch. 19 - Prob. 9SAQ Ch. 19 - Prob. 10SAQ

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