For an electrochemical cell 25oC with the following over-all reaction: Ag+(aq) + Br-(aq) → AgBr i. What should be the two half-reactions in its electrodes? ii. What is the short-hand notation for the cell? iii. What is the standard cell potential for the cell? iv. What is the cell potential and Gibbs fee energy change (∆G) of the cell if the concentration of AgBr solution is 0.05M (assuming activity of the solution is equal to its concentration)?
For an electrochemical cell 25oC with the following over-all reaction: Ag+(aq) + Br-(aq) → AgBr i. What should be the two half-reactions in its electrodes? ii. What is the short-hand notation for the cell? iii. What is the standard cell potential for the cell? iv. What is the cell potential and Gibbs fee energy change (∆G) of the cell if the concentration of AgBr solution is 0.05M (assuming activity of the solution is equal to its concentration)?
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
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 86E: An electrochemical cell consists of a silver metal electrode immersed in a solution with [Ag+] = 1.0...
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i. What should be the two half-reactions in its electrodes?
ii. What is the short-hand notation for the cell?
iii. What is the standard cell potential for the cell?
iv. What is the cell potential and Gibbs fee energy change (∆G) of the cell if the concentration of AgBr solution is 0.05M (assuming activity of the solution is equal to its concentration)?
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