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 Ag /Ag 1 [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.
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 Ag /Ag 1 [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.
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
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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2a
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PRE-LABORATORY ASSIGNMENT
Students must finish the pre-laboratory assignment before performing the laboratory experiment.
2.
1. An electrochemical cell comprises two electrodes: (Zn²+/Zn) and (Ag/Ag). Use the standard reduction
potentials to answer the following questions.
What is the standard potential of the cell?
b. Which electrode is the cathode, and which one is the anode?
a.
2. ElectroChemistry-2023-113.pdf
C.
Write a net redox equation for this electrochemical cell.
Consult the Appendix of "Principles of Modern Chemistry" by D. W. Oxtoby, H. P. Gillis, and Laurie J.
Butler for standard reduction potentials.
a.
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
To Do
1 85%
a 2 Û
1
[Ag*]
0
E = E 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?
183
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Transcribed Image Text:< Back
Calendar
PRE-LABORATORY ASSIGNMENT
Students must finish the pre-laboratory assignment before performing the laboratory experiment.
2.
1. An electrochemical cell comprises two electrodes: (Zn²+/Zn) and (Ag/Ag). Use the standard reduction
potentials to answer the following questions.
What is the standard potential of the cell?
b. Which electrode is the cathode, and which one is the anode?
a.
2. ElectroChemistry-2023-113.pdf
C.
Write a net redox equation for this electrochemical cell.
Consult the Appendix of "Principles of Modern Chemistry" by D. W. Oxtoby, H. P. Gillis, and Laurie J.
Butler for standard reduction potentials.
a.
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
To Do
1 85%
a 2 Û
1
[Ag*]
0
E = E 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?
183
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