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 110QRT
Related questions
Question
![1. (a) Balance the following simple redox reaction.
Fe (s) + O2(g) + 2H2O (I) Fe* + 4 OH
(b) If the standard change in the Gibbs energy of the molar reaction in part (a)
-507.13 kJ. Calculate the cell potential of the reaction.
2. Calculate the equilibrium constant at 25°C for the reaction
H2 + 2Fe 3+ 2H* + Fe2+
E° H'|H2 = 0.00 V and E° Fe3 |Fe2 = 0.771 V](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F65916b38-ab3b-40ec-97c0-4ccc1fad5366%2Fd5612cba-4ab8-4d51-b62b-8c13a1c1aef0%2Fpkydc1_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1. (a) Balance the following simple redox reaction.
Fe (s) + O2(g) + 2H2O (I) Fe* + 4 OH
(b) If the standard change in the Gibbs energy of the molar reaction in part (a)
-507.13 kJ. Calculate the cell potential of the reaction.
2. Calculate the equilibrium constant at 25°C for the reaction
H2 + 2Fe 3+ 2H* + Fe2+
E° H'|H2 = 0.00 V and E° Fe3 |Fe2 = 0.771 V
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