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.

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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.
Transcribed Image Text: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
Transcribed Image Text: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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