A current of 5.0 A was passed through an electrolytic cell containing molten BaCl2 for 90 min. The following redox reaction took place. 2 Cl– + Ba2+ → Cl2 + Ba MM of Ba = 137.3 g/mol MM of Cl2 = 70.9 g/mol R = 8.314 J/mol∙K F = 96,485 J/mol∙V A. How much product (in g) will be formed at the anode? B. How much product (in g) will be formed at the cathode?
A current of 5.0 A was passed through an electrolytic cell containing molten BaCl2 for 90 min. The following redox reaction took place. 2 Cl– + Ba2+ → Cl2 + Ba MM of Ba = 137.3 g/mol MM of Cl2 = 70.9 g/mol R = 8.314 J/mol∙K F = 96,485 J/mol∙V A. How much product (in g) will be formed at the anode? B. How much product (in g) will be formed at the cathode?
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 118AE
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A current of 5.0 A was passed through an electrolytic cell containing molten BaCl2 for 90 min. The following
2 Cl– + Ba2+ → Cl2 + Ba
MM of Ba = 137.3 g/mol
MM of Cl2 = 70.9 g/mol
R = 8.314 J/mol∙K
F = 96,485 J/mol∙V
A. How much product (in g) will be formed at the anode?
B. How much product (in g) will be formed at the cathode?
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