A current of 0.600 A is passed through an electrolytic cell containing molten KBr for 2.50 h. How much product will be formed at the anode? 2Br + 2K+ → Br₂ + 2K MM of K = 39.10 g/mol MM of Br₂ = 159.8 g/mol R = 8.314 J/mol-K F = 96,485 J/mol-V O 1.09 g O 4.47 g O 8.94 g O 2.19 g

A current of 0.600 A is passed through an electrolytic cell containing molten KBr for 2.50 h. How much product will be formed at the anode? 2Br + 2K+ → Br₂ + 2K MM of K = 39.10 g/mol MM of Br₂ = 159.8 g/mol R = 8.314 J/mol-K F = 96,485 J/mol-V O 1.09 g O 4.47 g O 8.94 g O 2.19 g

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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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

A current of 0.600 A is passed through an electrolytic cell containing molten KBr
for 2.50 h. How much product will be formed at the anode?
2Br + 2K+ → Br₂ + 2K
MM of K = 39.10 g/mol
MM of Br₂ = 159.8 g/mol
R = 8.314 J/mol-K
F = 96,485 J/mol-V
O 1.09 g
O 4.47 g
O 8.94 g
O 2.19 g

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