Calculate the quantity of charge necessary to produce 5.0 liters of H 2(g) at 25 C and 1 atm from the electrolysis of water. O a. 4.3 x 104 coulombs O b.8.6 x 104 coulombs O c. 3.7 x 104 coulombs O d.2.7 x 104 coulombs O e. 5.5x 104 coulombs

Calculate the quantity of charge necessary to produce 5.0 liters of H 2(g) at 25 C and 1 atm from the electrolysis of water. O a. 4.3 x 104 coulombs O b.8.6 x 104 coulombs O c. 3.7 x 104 coulombs O d.2.7 x 104 coulombs O e. 5.5x 104 coulombs

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 100E: A factory wants to produce 1.00 103 kg barium from the electrolysis of molten barium chloride. What...

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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 quantity of charge necessary to produce 5.0 liters of H 2(g) at 25 C and 1 atm from the electrolysis of water.
Oa. 4.3 x 104 coulombs
O b.8.6 x 104 coulombs
c. 3.7 x 104 coulombs
O d.2.7 x 104 coulombs
O e. 5.5 x 104 coulombs

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