2. You are given an electrochemical cell where the chemical reaction involves a silver complex, and a silver metal bar is provided as the positive electrode. The electrochemical potential for this cell is given by a. E=Eº 1 [Ag*] Ag /Ag -0.0592(volts)-log- For a test solution with a silver concentration of 0.001 M, the electrochemical cell potential is 0.20 volts. Find the silver electrode potential EºAg+/Ag- b. This same cell from (a) is used to measure the electrochemical potential for a new silver complex in equilibrium. If the measured cell potential is 0.324 volts, what is the silver concentration for this new silver complex at a chemical equilibrium state?
2. You are given an electrochemical cell where the chemical reaction involves a silver complex, and a silver metal bar is provided as the positive electrode. The electrochemical potential for this cell is given by a. E=Eº 1 [Ag*] Ag /Ag -0.0592(volts)-log- For a test solution with a silver concentration of 0.001 M, the electrochemical cell potential is 0.20 volts. Find the silver electrode potential EºAg+/Ag- b. This same cell from (a) is used to measure the electrochemical potential for a new silver complex in equilibrium. If the measured cell potential is 0.324 volts, what is the silver concentration for this new silver complex at a chemical equilibrium state?
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 77AP
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