2. Did the reduced concentration of Cu²+ ion in the cells using the 0.5 M Cu(NO3)₂ and 0.1 MCu(NO3), solutions affect the cell potentials? If there is an effect, please suggest an explanation. 4.NameEXPERIMENT 12ELECTROCHEMISTRY: GALVANIC CELLSElectrodesUse the table of standard reduction potentials from your textbook to complete the following table.The zinc-copper Daniell cell is given as an example.CuCuZnZnZnCuZnMgCuMgConc. ofEach Cation1.0 M Zn²+0.5 M Cu²+1.0 M Zn²+0.1 M Cu²+Date1.0 M Zn²+Zn²+ + 2e-Zn(ag)Half-ReactionsA. Determine the E for the Standard Zn-Cu Galvanic CellZn²+(aq)1.0 M Cu²+Cu²++2e-CuCathodeB. Determine the E* for the Cu-Zn Cell at Non-standard Concentrations1.0 M Zn²+Anode+ 2e → ZnInstructorCu²+2e-CuZn²+ + 2e → Zn(aq)Report SheetCathode orAnode?AnodeEE(table) (calcd)-0.76 V+0.34 V-0.76VCathode 0.34 vanode 0.76vCathode 0.34 vCu²+ + 2e - CulC. Determine the E for Zn-Mg and Cu-Mg Galvanic CellsZn(aq) +2e Zn (s) cathode -0.761.0 M Mg²+Mga+2e Mg(s) anode -2.38+1.10 V1.10 V1.0 M Cu²+ +Ze Cu(s) Cathode 40.34 v2+ +2e1.0 M Mg²+ MMg(s) anode -2.38v"You must use the Nernst equation to calculate this Ecell voltage. (See Equation 8.)1.62 v1.10 0.98 vEº(measured)2.72v+1.06 x1.04 v1.54 v1.99 vVELECTROCHEMISTRY: GALVANIC CELLS 141M

We need to explain does the reduced concentration of Cu2+ ion varies with different concentration of solution.The reduction potential of an electrode depends upon the concentration of solution with which the electrode is emerged in. This can be explained through Nernst equation. For instance, A reduction half-reaction for Cu2+|Cu cell is written as follows: Cu2+ aq + 2e → Cu s The Nernst equation for the above reaction is given as: Ered half reaction = ECu2+/Cuo - RT2Fln1Cu2+Ered half reaction = ECu2+/Cuo + RT2FlnCu2+ This implies that the concentration of solution depends upon the concentration of Cu2+ ions. Hence, 0.5 M and 0.1 M Cu(NO3)2 solutions will have different reduction potential values as it strongly depends on the concentration of Cu2+ ions.

Answered: Did the reduced concentration of Cu²+…

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Did the reduced concentration of Cu²+ ion in the cells using the 0.5 M Cu(NO3), and 0.1 M Cu(NO3), solutions affect the cell potentials? If there is an effect, please suggest an explanation.

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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Question

2. Did the reduced concentration of Cu²+ ion in the cells using the 0.5 M Cu(NO3)₂ and 0.1 M
Cu(NO3), solutions affect the cell potentials? If there is an effect, please suggest an explanation.

4.
Name
EXPERIMENT 12
ELECTROCHEMISTRY: GALVANIC CELLS
Electrodes
Use the table of standard reduction potentials from your textbook to complete the following table.
The zinc-copper Daniell cell is given as an example.
Cu
Cu
Zn
Zn
Zn
Cu
Zn
Mg
Cu
Mg
Conc. of
Each Cation
1.0 M Zn²+
0.5 M Cu²+
1.0 M Zn²+
0.1 M Cu²+
Date
1.0 M Zn²+
Zn²+ + 2e-Zn
(ag)
Half-Reactions
A. Determine the E for the Standard Zn-Cu Galvanic Cell
Zn²+
(aq)
1.0 M Cu²+
Cu²+
+2e-Cu
Cathode
B. Determine the E* for the Cu-Zn Cell at Non-standard Concentrations
1.0 M Zn²+
Anode
+ 2e → Zn
Instructor
Cu²+2e-Cu
Zn²+ + 2e → Zn
(aq)
Report Sheet
Cathode or
Anode?
Anode
E
E
(table) (calcd)
-0.76 V
+0.34 V
-0.76V
Cathode 0.34 v
anode 0.76v
Cathode 0.34 v
Cu²+ + 2e - Cul
C. Determine the E for Zn-Mg and Cu-Mg Galvanic Cells
Zn(aq) +2e Zn (s) cathode -0.76
1.0 M Mg²+Mga+2e Mg(s) anode -2.38
+1.10 V
1.10 V
1.0 M Cu²+ +Ze Cu(s) Cathode 40.34 v
2+ +2e
1.0 M Mg²+ M
Mg(s) anode -2.38v
"You must use the Nernst equation to calculate this Ecell voltage. (See Equation 8.)
1.62 v
1.10 0.98 v
Eº
(measured)
2.72v
+1.06 x
1.04 v
1.54 v
1.99 v
V
ELECTROCHEMISTRY: GALVANIC CELLS 141
M

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