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Electrode systems used in cell 2n/Zn²+ Cul Cuat 2. Zn/Znat Fe²+ Fest 3. Cu/cuat AS/Agr 4.Zn/Zn²+ Ag/Agr 5. Zn/Zn2+ 1₂/I- 6. Fe2+ ke st Bra Br at 7. Br₂/Br Cia 101 Calculations Cell potential, Ecell (volts) .83 41 .41 1.3 1.0 .41 .10 Negative electrode Zn zn си 2n Zn Fe CI Oxidation reaction Exidation in volts Reduction reaction EⓇ Preduction in volts A. Noting that oxidation occurs at the negative pole in a cell, write the oxidation reaction taking place in each of the cells. The other electrode system must undergo reduction; write the reduction reaction that occurs in each cell. B. Assume that E AB = 0.00 volts (whether in reduction or oxidation). Enter that value in the table for all of the silver electrode systems you used in your cells. Since Ecell = Eoxidation +Ereduction you can calculate Eº values for all the electrode systems in which the Ag.Ag system was involved. Enter those values in the table. C. Using the values and relations in Part B and taking advantage of the fact that for any given electrode system, Eoxidation=-Eroduction complete the table of E values. The best way to do this is to use one of the E values you found in Part B in another cell with that electrode system. That potential, along with Ell, will allow you to find the potential of the other electrode. Continue this process with other cells until all the electrode potentials have been determined.

Electrode systems used in cell 2n/Zn²+ Cul Cuat 2. Zn/Znat Fe²+ Fest 3. Cu/cuat AS/Agr 4.Zn/Zn²+ Ag/Agr 5. Zn/Zn2+ 1₂/I- 6. Fe2+ ke st Bra Br at 7. Br₂/Br Cia 101 Calculations Cell potential, Ecell (volts) .83 41 .41 1.3 1.0 .41 .10 Negative electrode Zn zn си 2n Zn Fe CI Oxidation reaction Exidation in volts Reduction reaction EⓇ Preduction in volts A. Noting that oxidation occurs at the negative pole in a cell, write the oxidation reaction taking place in each of the cells. The other electrode system must undergo reduction; write the reduction reaction that occurs in each cell. B. Assume that E AB = 0.00 volts (whether in reduction or oxidation). Enter that value in the table for all of the silver electrode systems you used in your cells. Since Ecell = Eoxidation +Ereduction you can calculate Eº values for all the electrode systems in which the Ag.Ag system was involved. Enter those values in the table. C. Using the values and relations in Part B and taking advantage of the fact that for any given electrode system, Eoxidation=-Eroduction complete the table of E values. The best way to do this is to use one of the E values you found in Part B in another cell with that electrode system. That potential, along with Ell, will allow you to find the potential of the other electrode. Continue this process with other cells until all the electrode potentials have been determined.

Chemistry
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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Please complete Table A1.

A.1. Cell Potentials Electrode systems used in cell 2nl Zn²+ Cul Cuat 2. Zn/Znat Fest Fest 3. Cu/cuat AS/Agr 4.Zn/Zn²+ Ag/Agr 5. Zn/2h27 I₂/I- 6. Fe2+ ke 3+ Bra Br 7. Bra / Br Cia 101 Calculations Cell potential, Ecell (volts) .83 .41 .41 1.3 1.0 .41 .10 Negative electrode zn zn си 2n Zn Fe CI Oxidation reaction E Foxidation in volts Reduction reaction Ereduction in volts A. Noting that oxidation occurs at the negative pole in a cell, write the oxidation reaction taking place in each of the cells. The other electrode system must undergo reduction; write the reduction reaction that occurs in each cell. B. Assume that E Ag-Ag = 0.00 volts (whether in reduction or oxidation). Enter that value in the table for all of the silver electrode systems you used in your cells. Since Ecell = Eoxidation +Ereductions you can calculate Eº values for all the electrode systems in which the Ag.Ag system was involved. Enter those values in the table. C. Using the values and relations in Part B and taking advantage of the fact that for any given electrode system, Exidation =-Eroductions complete the table of E values. The best way to do this is to use one of the Eº values you found in Part B in another cell with that electrode system. That potential, along with Ell, will allow you to find the potential of the other electrode. Continue this process with other cells until all the electrode potentials have been determined. (continued on following page) Data and Calculations: Voltaic Cell Measurements. Experiment 32
Transcribed Image Text:A.1. Cell Potentials Electrode systems used in cell 2nl Zn²+ Cul Cuat 2. Zn/Znat Fest Fest 3. Cu/cuat AS/Agr 4.Zn/Zn²+ Ag/Agr 5. Zn/2h27 I₂/I- 6. Fe2+ ke 3+ Bra Br 7. Bra / Br Cia 101 Calculations Cell potential, Ecell (volts) .83 .41 .41 1.3 1.0 .41 .10 Negative electrode zn zn си 2n Zn Fe CI Oxidation reaction E Foxidation in volts Reduction reaction Ereduction in volts A. Noting that oxidation occurs at the negative pole in a cell, write the oxidation reaction taking place in each of the cells. The other electrode system must undergo reduction; write the reduction reaction that occurs in each cell. B. Assume that E Ag-Ag = 0.00 volts (whether in reduction or oxidation). Enter that value in the table for all of the silver electrode systems you used in your cells. Since Ecell = Eoxidation +Ereductions you can calculate Eº values for all the electrode systems in which the Ag.Ag system was involved. Enter those values in the table. C. Using the values and relations in Part B and taking advantage of the fact that for any given electrode system, Exidation =-Eroductions complete the table of E values. The best way to do this is to use one of the Eº values you found in Part B in another cell with that electrode system. That potential, along with Ell, will allow you to find the potential of the other electrode. Continue this process with other cells until all the electrode potentials have been determined. (continued on following page) Data and Calculations: Voltaic Cell Measurements. Experiment 32
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