5. What effect, if any, would varying the concentration of both the aqueous species have on thecell potentials? What about varying the size of the electrodes? 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

On changing the concentration ,changes can be observed in the E° measured values. This can be shown by Nernst equation. Let us consider the change in concentration of cathode in each case, As we can see that on changing concentration of any one electrode , the E°calc. changes . The size of electrodes do not have any effect on cell potential. Rather size of the electrodes changes the resistance only.

Answered: 5. What effect, if any, would varying…

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5. What effect, if any, would varying the concentration of both the aqueous species have on the cell potentials? What about varying the size of the electrodes?

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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

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Question

5. What effect, if any, would varying the concentration of both the aqueous species have on the
cell potentials? What about varying the size of the electrodes?

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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