Cell Zn-Cu EXP. 3 VOLTAIC CELLS POST-LAB REPORT WORKSHEETS Part 2- Measurement of Cell Potentials 1. Note: Because [Fe²] 0.5 M, the experimental voltages can be expected to. deviate from the calculated voltages (using the Nernst equation) where Fe²+ half-cells are involved. Experimental Voltage Readings and Average 1.092 + 1.092 2 = 1.095 V 0.465 +0.465 At which metal does reduction occur? Cu Cilt (agite -Cu +0.16V At which metal does oxidation occur? Zn 2n ² (a) + 2é → zn (s) -0.76V Pi Which metal is the stronger reducing agent? 2n -076 V PI Calculated Voltage (assume 0.5 M)
Cell Zn-Cu EXP. 3 VOLTAIC CELLS POST-LAB REPORT WORKSHEETS Part 2- Measurement of Cell Potentials 1. Note: Because [Fe²] 0.5 M, the experimental voltages can be expected to. deviate from the calculated voltages (using the Nernst equation) where Fe²+ half-cells are involved. Experimental Voltage Readings and Average 1.092 + 1.092 2 = 1.095 V 0.465 +0.465 At which metal does reduction occur? Cu Cilt (agite -Cu +0.16V At which metal does oxidation occur? Zn 2n ² (a) + 2é → zn (s) -0.76V Pi Which metal is the stronger reducing agent? 2n -076 V PI Calculated Voltage (assume 0.5 M)
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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![Cell
Zn-Cu
Cu-Pb
Cu-Fe
Zn-Pb
Fe-Zn
Fe-Pb
EXP. 3 VOLTAIC CELLS
POST-LAB REPORT WORKSHEETS
Part 2 - Measurement of Cell Potentials
1. Note: Because [Fe²] # 0.5 M, the experimental voltages can be expected to
deviate from the calculated voltages (using the Nernst equation) where Fe²+
half-cells are involved.
Experimental
Voltage
Readings and
Average
1.092+ 1,012
2
= 1.095 V
0.465 +0.465
2
= 0.465 V
0.028 +0027
C
= 00275V
0.650+ 0.628
0.629 V
0.321 +0,322
2
= 0.3215 V
0.002 0.004
"
= 0.003 V
At which metal
does reduction
occur?
Cn
Cult (agite
→ Cut
Си
+0.16V
Си
+0.16V
+0.16 V
Zn
-0.76V
2n
-0.76
Pb
At which metal
does oxidation
occur?
-0.131
Zn
Zn ² (a) + 2é
→ zn (s)
-0.76V
Pb
-0.13V
Fe
Pb
+0.77V
-0.13V
Fe
+0.77 V
Fe
Which metal is
the stronger
reducing
agent?
2n
-076 V
Pb
-0.13V
Fe
+0.77V
Pb
-0.13 V
Fe
+0.77
Fe
Calculated
Voltage
(assume 0.5 M)
+0.77
+0.77
2. On the basis of the calculated voltages, write the order for the reducing strength
of the four metals (Zn, Cu, Pb, Fe), in order of decreasing reducing strength.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9d766829-6e63-418a-a7ad-7ecbe0097428%2Fef4816f8-1531-4cb7-86ae-c42f21fc7a0d%2Fffqk15d_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Cell
Zn-Cu
Cu-Pb
Cu-Fe
Zn-Pb
Fe-Zn
Fe-Pb
EXP. 3 VOLTAIC CELLS
POST-LAB REPORT WORKSHEETS
Part 2 - Measurement of Cell Potentials
1. Note: Because [Fe²] # 0.5 M, the experimental voltages can be expected to
deviate from the calculated voltages (using the Nernst equation) where Fe²+
half-cells are involved.
Experimental
Voltage
Readings and
Average
1.092+ 1,012
2
= 1.095 V
0.465 +0.465
2
= 0.465 V
0.028 +0027
C
= 00275V
0.650+ 0.628
0.629 V
0.321 +0,322
2
= 0.3215 V
0.002 0.004
"
= 0.003 V
At which metal
does reduction
occur?
Cn
Cult (agite
→ Cut
Си
+0.16V
Си
+0.16V
+0.16 V
Zn
-0.76V
2n
-0.76
Pb
At which metal
does oxidation
occur?
-0.131
Zn
Zn ² (a) + 2é
→ zn (s)
-0.76V
Pb
-0.13V
Fe
Pb
+0.77V
-0.13V
Fe
+0.77 V
Fe
Which metal is
the stronger
reducing
agent?
2n
-076 V
Pb
-0.13V
Fe
+0.77V
Pb
-0.13 V
Fe
+0.77
Fe
Calculated
Voltage
(assume 0.5 M)
+0.77
+0.77
2. On the basis of the calculated voltages, write the order for the reducing strength
of the four metals (Zn, Cu, Pb, Fe), in order of decreasing reducing strength.
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