Consider the hydrolysis of pure water (an electrolytic cell): Anode: 2 H2O(l ) → O2(g ) + 4 H+(aq ) + 4 e− E° = −1.23 V Cathode: 2 H2O(l ) + 2 e− → H2(g ) + 2 OH−(aq ) E° = −0.83 V True or False: Hydrolysis can do work. Group of answer choices True False
Consider the hydrolysis of pure water (an electrolytic cell): Anode: 2 H2O(l ) → O2(g ) + 4 H+(aq ) + 4 e− E° = −1.23 V Cathode: 2 H2O(l ) + 2 e− → H2(g ) + 2 OH−(aq ) E° = −0.83 V True or False: Hydrolysis can do work. Group of answer choices True False
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
Section: Chapter Questions
Problem 59QRT: Consider the electrolysis of water in the presence of very dilute H2SO4. What species is produced at...
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Consider the hydrolysis of pure water (an electrolytic cell):
Anode: 2 H2O(l ) → O2(g ) + 4 H+(aq ) + 4 e− E° = −1.23 V
Cathode: 2 H2O(l ) + 2 e− → H2(g ) + 2 OH−(aq ) E° = −0.83 V
True or False: Hydrolysis can do work.
Group of answer choices
True
False
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