1. Use the identities of the anode and cathode to give the overall cell reaction for each voltaic cell. 2. b. Use the Nernst equation, where necessary, to calculate E°cell for each overall cell reaction. Studying the Other Voltaic Cells1.You may begin this part of the experiment while the electrolysis is progressing. These studies canbe interrupted when the electrolysis is completed.2.After you have read all of the instructions, determine the anodes, cathodes, and voltages of thefollowing voltaic cells:Cu²+ | Cu and Pb²+ | PbCu²+ | Cu and Fe²+ | FeCu²+ | Cu and Fe³+, Fe²+ | Pt (or graphite)Zn²+ | Zn and Pb²+ PbZn²+ Zn and Fe²+ | Fea.b.C.d.e.f.g.Zn²+ | Zn and Fe³+, Fe²+ | Pt (or graphite)Fe²+ Fe and Fe³+, Fe²+ | Pt (or graphite)Copyright 2017 Cengage Learning. All Rights Reserved. May not be copied, scanned, or duplicated, in whole or in par. Due to electronic rights, some third party content may be suppressed from the eBook ander Chapters)rial review has deemed that any suppressed content does not materially affect the overall leaming experience. Cengage Leaming reserves the right to remove additional content at any time if subsequent rights restrictions requireit.Experiment 19BIf you are using a salt bridge, also includeh.Pb²+ | Pb and Fe² | Fei. Pb²+ | Pb and Fe, Fe²* | Pt (or graphite)You should not study these two cells if you are using a porous pot, a porous glass plug, or amembrane because the precipitation of PbSO4, which can occur at the junction of the solutions,would plug the pores of these pieces of equipment and cause errors in your results.The solutions that are to be used for these voltaic cells are 0.10 M solutions of Zn(NO3)2,Pb(NO3)2, FeSO4(stored over iron wire or nails), and Cu(NO3)2, along with an iron solutioncomposed of 0.050 M FeSO4 and 0.050 M Fe2(SO4)3 in 1 M H₂SO4.Prepare the copper, iron, lead, and zinc electrodes by cleaning, rinsing, and drying them accordingto the directions given previously.CAUTION: When you have completed this part of theexperiment, wash your hands. Solutions containing lead are 3.Other voltaic cellsCu 2+Cu2+Cu2+Zn2+Zn2+Zn2+Fe2+Pb2+Pb2+ElectrodesPbFePtPbFegraphitegraphiteFegraphiteCell Potential (V)0.4890.5740.4280.4770.3451.3210.9960.1440.841AnodeFePbCuZnZnZnFeFePbCathodeCuCugraphiteCuFegraphitegraphitePbgraphite

Nernst equation will be represented as, Ecell = E0cell - RTnFlog[anode][cathode] Ecell = electrode…

Answered: 1. You may begin this part of the…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 93QRT

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Question

1. Use the identities of the anode and cathode to give the overall cell reaction for each voltaic cell. 2. b. Use the Nernst equation, where necessary, to calculate E°cell for each overall cell reaction.

Studying the Other Voltaic Cells
1.
You may begin this part of the experiment while the electrolysis is progressing. These studies can
be interrupted when the electrolysis is completed.
2.
After you have read all of the instructions, determine the anodes, cathodes, and voltages of the
following voltaic cells:
Cu²+ | Cu and Pb²+ | Pb
Cu²+ | Cu and Fe²+ | Fe
Cu²+ | Cu and Fe³+, Fe²+ | Pt (or graphite)
Zn²+ | Zn and Pb²+ Pb
Zn²+ Zn and Fe²+ | Fe
a.
b.
C.
d.
e.
f.
g.
Zn²+ | Zn and Fe³+, Fe²+ | Pt (or graphite)
Fe²+ Fe and Fe³+, Fe²+ | Pt (or graphite)
Copyright 2017 Cengage Learning. All Rights Reserved. May not be copied, scanned, or duplicated, in whole or in par. Due to electronic rights, some third party content may be suppressed from the eBook ander Chapters)
rial review has deemed that any suppressed content does not materially affect the overall leaming experience. Cengage Leaming reserves the right to remove additional content at any time if subsequent rights restrictions requireit.
Experiment 19B
If you are using a salt bridge, also include
h.
Pb²+ | Pb and Fe² | Fe
i. Pb²+ | Pb and Fe, Fe²* | Pt (or graphite)
You should not study these two cells if you are using a porous pot, a porous glass plug, or a
membrane because the precipitation of PbSO4, which can occur at the junction of the solutions,
would plug the pores of these pieces of equipment and cause errors in your results.
The solutions that are to be used for these voltaic cells are 0.10 M solutions of Zn(NO3)2,
Pb(NO3)2, FeSO4(stored over iron wire or nails), and Cu(NO3)2, along with an iron solution
composed of 0.050 M FeSO4 and 0.050 M Fe2(SO4)3 in 1 M H₂SO4.
Prepare the copper, iron, lead, and zinc electrodes by cleaning, rinsing, and drying them according
to the directions given previously.
CAUTION: When you have completed this part of the
experiment, wash your hands. Solutions containing lead are

3.
Other voltaic cells
Cu 2+
Cu2+
Cu2+
Zn2+
Zn2+
Zn2+
Fe2+
Pb2+
Pb2+
Electrodes
Pb
Fe
Pt
Pb
Fe
graphite
graphite
Fe
graphite
Cell Potential (V)
0.489
0.574
0.428
0.477
0.345
1.321
0.996
0.144
0.841
Anode
Fe
Pb
Cu
Zn
Zn
Zn
Fe
Fe
Pb
Cathode
Cu
Cu
graphite
Cu
Fe
graphite
graphite
Pb
graphite

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Can the ones with graphite be done with graphite instead. . Use the identities of the anode and cathode to give the overall cell reaction for each voltaic cell.

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Show that your experimental results are in agreement with the following statements about reactions that occur outside of a voltaic cell. a. Zn will reduce Cu2+ ions, but Zn2+ ions are not reduced by Cu. b. Fe2+ ions are not oxidized by Zn2+ ions. c. When an iron nail is inserted into a solution of Cu2+ ions, metallic copper is deposited on the nail. d. When a piece of lead is inserted into a solution of Zn2+ ions, no reaction occurs. 5. a. Calculate the expected cell potential from the copper concentration cell before the addition of 0.10 M Cu(NO3)2.

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