A 0.100 M neutral aqueous CaCl2 solution is electrolyzed using platinum electrodes. A current of 1.50 A passes through the solution for 50.0 hours.(a) Write the half-reactions occurring at the anode and at the cathode.(b) What is the decomposition potential?(c) Calculate the mass, in grams, of the product formed at the cathode.
A 0.100 M neutral aqueous CaCl2 solution is electrolyzed using platinum electrodes. A current of 1.50 A passes through the solution for 50.0 hours.(a) Write the half-reactions occurring at the anode and at the cathode.(b) What is the decomposition potential?(c) Calculate the mass, in grams, of the product formed at the cathode.
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 97AP
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A 0.100 M neutral aqueous CaCl2 solution is electrolyzed using platinum electrodes. A current of 1.50 A passes through the solution for 50.0 hours.
(a) Write the half-reactions occurring at the anode and at the cathode.
(b) What is the decomposition potential?
(c) Calculate the mass, in grams, of the product formed at the cathode.
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