1. You may begin this part of the experiment while the electrolysis is progressing. These studies 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 Fe*, Fe² | Pt (or graphite) Zn²+ Zn and Pb²+|Pb Zn²+ Zn and Fe²+ | Fe a. b. C. d. e. f. Zn²+ | Zn and Fe³+, Fe²+ | Pt (or graphite) g. Fe| Fe and Fe³+, Fe² | Pt (or graphite) ight 2017 Cengage Leaming. All Rights Reserved. May not be copied, sesed, or delicated, in whole or in pat. Due to electronic sights, see this party content may be suppressed from the eBook ander Chapters) niew 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 requi you are using a salt bridge, also include Pb²+ | Pb and Fe²+ | Fe Pb² | Pb and Fe, Fe² | Pt (or graphite) Experiment 19B

Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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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
Transcribed Image Text: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
Transcribed Image Text: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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Follow-up Question

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.

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
Transcribed Image Text: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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Follow-up Question

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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