Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 18 minutes at a current of 2.8 A given the following reaction. Z3+(aq) + 3e- Z(s) Atomic Mass: Z: 182.35 g/mol Round your answer to 2 decimal places.

Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 18 minutes at a current of 2.8 A given the following reaction. Z3+(aq) + 3e- Z(s) Atomic Mass: Z: 182.35 g/mol Round your answer to 2 decimal places.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section17.11: Counting Electrons

Problem 17.19E

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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.

Question

Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 18
minutes at a current of 2.8 A given the following reaction.
Z3*(aq) + 3e- → Z(s)
Atomic Mass:
Z: 182.35 g/mol
Round your answer to 2 decimal places.

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