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4. Compare the sum of the Cu-Zn and the Zn-Mg cell potentials with the Cu-Mg cell potential. What can you conclude? 5. What effect, if any, would varying the concentration of both the aqueous species have on the cell potentials? What about varying the size of the electrodes?

4. Compare the sum of the Cu-Zn and the Zn-Mg cell potentials with the Cu-Mg cell potential. What can you conclude? 5. What effect, if any, would varying the concentration of both the aqueous species have on the cell potentials? What about varying the size of the electrodes?

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
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4. Compare the sum of the Cu-Zn and the Zn-Mg cell potentials with the Cu-Mg cell potential. What can you conclude? 5. What effect, if any, would varying the concentration of both the aqueous species have on the cell potentials? What about varying the size of the electrodes? 144 EXPERIMENT 12 PA K (4
Transcribed Image Text:4. Compare the sum of the Cu-Zn and the Zn-Mg cell potentials with the Cu-Mg cell potential. What can you conclude? 5. What effect, if any, would varying the concentration of both the aqueous species have on the cell potentials? What about varying the size of the electrodes? 144 EXPERIMENT 12 PA K (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 Zn Zn Zn Cu Cu Zn Mg Cu Mg Conc. of Each Cation 1.0 M Zn²+ 1.0 M Cu²+ 0.5 M Cu²+ 1.0 M Zn²+ Date 0.1 M Cu²+ Zn²+ + 2e-Zn (ag) Instructor Cu²+2e-Cu B. Determine the E* for the Cu-Zn Cell at Non-standard Concentrations Anode 0.46 V 1.0 M Zn²+ Cu²+ + 2e-Cu Half-Reactions A. Determine the E for the Standard Zn-Cu Galvanic Cell Zn²+ + 2e-Zn -0.76 V Zn²+ + 2e- → Zn Cathode or Anode? +2e Report Sheet Anode E E (table) (calc'd) Cathode +0.34 V Cathode 0.34 v anode 0.76 1.0 M Zn²+ Zn (aq) +2e-Zn (s) 1.0 M Mg²+Mga+2e Mg (s) 1.0 M Cu²+C+Ze Cu(s) 1.0 M Mg²+ M Mg(s) "You must use the Nernst equation to calculate this Ecell voltage. (See Equation 8.) Cathode 0.34 v Cu²+ + 2e → Cu C. Determine the E for Zn-Mg and Cu-Mg Galvanic Cells Cathode -0.76 anode -2.38v +1.10 V 1.06 v Cathode 0.34v arode -2.38v 1.10 1.04 v E (measured) 1.10 0.98 v 1.62 v ? 1.54 v 2.72 1.98v ELECTROCHEMISTRY: GALVANIC CELLS 141 9 PgUp 6 3 PgDn Del C Backs Pad + Ent
Transcribed Image Text: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 Zn Zn Zn Cu Cu Zn Mg Cu Mg Conc. of Each Cation 1.0 M Zn²+ 1.0 M Cu²+ 0.5 M Cu²+ 1.0 M Zn²+ Date 0.1 M Cu²+ Zn²+ + 2e-Zn (ag) Instructor Cu²+2e-Cu B. Determine the E* for the Cu-Zn Cell at Non-standard Concentrations Anode 0.46 V 1.0 M Zn²+ Cu²+ + 2e-Cu Half-Reactions A. Determine the E for the Standard Zn-Cu Galvanic Cell Zn²+ + 2e-Zn -0.76 V Zn²+ + 2e- → Zn Cathode or Anode? +2e Report Sheet Anode E E (table) (calc'd) Cathode +0.34 V Cathode 0.34 v anode 0.76 1.0 M Zn²+ Zn (aq) +2e-Zn (s) 1.0 M Mg²+Mga+2e Mg (s) 1.0 M Cu²+C+Ze Cu(s) 1.0 M Mg²+ M Mg(s) "You must use the Nernst equation to calculate this Ecell voltage. (See Equation 8.) Cathode 0.34 v Cu²+ + 2e → Cu C. Determine the E for Zn-Mg and Cu-Mg Galvanic Cells Cathode -0.76 anode -2.38v +1.10 V 1.06 v Cathode 0.34v arode -2.38v 1.10 1.04 v E (measured) 1.10 0.98 v 1.62 v ? 1.54 v 2.72 1.98v ELECTROCHEMISTRY: GALVANIC CELLS 141 9 PgUp 6 3 PgDn Del C Backs Pad + Ent
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