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1. Based on your observations: a. Which cell produces the highest cell potential? Explain. b. Which cell produces the lowest cell potential? Explain.

1. Based on your observations: a. Which cell produces the highest cell potential? Explain. b. Which cell produces the lowest cell potential? Explain.

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 77AP
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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 Cu Zn Zn Zn Cu Zn Mg Cu Mg Conc. of Each Cation 1.0 M Zn²+ 0.5 M Cu²+ 1.0 M Zn²+ 0.1 M Cu²+ Date 1.0 M Zn²+ Zn²+ + 2e-Zn (ag) Half-Reactions A. Determine the E for the Standard Zn-Cu Galvanic Cell Zn²+ (aq) 1.0 M Cu²+ Cu²+ +2e-Cu Cathode B. Determine the E* for the Cu-Zn Cell at Non-standard Concentrations 1.0 M Zn²+ Anode + 2e → Zn Instructor Cu²+2e-Cu Zn²+ + 2e → Zn (aq) Report Sheet Cathode or Anode? Anode E E (table) (calcd) -0.76 V +0.34 V -0.76V Cathode 0.34 v anode 0.76v Cathode 0.34 v Cu²+ + 2e - Cul C. Determine the E for Zn-Mg and Cu-Mg Galvanic Cells Zn(aq) +2e Zn (s) cathode -0.76 1.0 M Mg²+Mga+2e Mg(s) anode -2.38 +1.10 V 1.10 V 1.0 M Cu²+ +Ze Cu(s) Cathode 40.34 v 2+ +2e 1.0 M Mg²+ M Mg(s) anode -2.38v "You must use the Nernst equation to calculate this Ecell voltage. (See Equation 8.) 1.62 v 1.10 0.98 v Eº (measured) 2.72v +1.06 x 1.04 v 1.54 v 1.99 v V ELECTROCHEMISTRY: GALVANIC CELLS 141 M
Transcribed Image Text: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 Cu Zn Zn Zn Cu Zn Mg Cu Mg Conc. of Each Cation 1.0 M Zn²+ 0.5 M Cu²+ 1.0 M Zn²+ 0.1 M Cu²+ Date 1.0 M Zn²+ Zn²+ + 2e-Zn (ag) Half-Reactions A. Determine the E for the Standard Zn-Cu Galvanic Cell Zn²+ (aq) 1.0 M Cu²+ Cu²+ +2e-Cu Cathode B. Determine the E* for the Cu-Zn Cell at Non-standard Concentrations 1.0 M Zn²+ Anode + 2e → Zn Instructor Cu²+2e-Cu Zn²+ + 2e → Zn (aq) Report Sheet Cathode or Anode? Anode E E (table) (calcd) -0.76 V +0.34 V -0.76V Cathode 0.34 v anode 0.76v Cathode 0.34 v Cu²+ + 2e - Cul C. Determine the E for Zn-Mg and Cu-Mg Galvanic Cells Zn(aq) +2e Zn (s) cathode -0.76 1.0 M Mg²+Mga+2e Mg(s) anode -2.38 +1.10 V 1.10 V 1.0 M Cu²+ +Ze Cu(s) Cathode 40.34 v 2+ +2e 1.0 M Mg²+ M Mg(s) anode -2.38v "You must use the Nernst equation to calculate this Ecell voltage. (See Equation 8.) 1.62 v 1.10 0.98 v Eº (measured) 2.72v +1.06 x 1.04 v 1.54 v 1.99 v V ELECTROCHEMISTRY: GALVANIC CELLS 141 M
*- R F 15 % V + T G 6 NNNNNNA Name EXPERIMENT 12 ELECTROCHEMISTRY: GALVANIC CELLS Date Post-Laboratory Questions 1. Based on your observations: a. Which cell produces the highest cell potential? Explain. b. Which cell produces the lowest cell potential? Explain. Instructor 2. Did the reduced concentration of Cu²+ ion in the cells using the 0.5 M Cu(NO), and 0.1 M Cu(NO), solutions affect the cell potentials? If there is an effect, please suggest an explanation. 3. What is the oxidizing agent in the Zn-Mg cell? ELECTROCHEMISTRY: GALVANIC CELLS 143 E15 nter
Transcribed Image Text:*- R F 15 % V + T G 6 NNNNNNA Name EXPERIMENT 12 ELECTROCHEMISTRY: GALVANIC CELLS Date Post-Laboratory Questions 1. Based on your observations: a. Which cell produces the highest cell potential? Explain. b. Which cell produces the lowest cell potential? Explain. Instructor 2. Did the reduced concentration of Cu²+ ion in the cells using the 0.5 M Cu(NO), and 0.1 M Cu(NO), solutions affect the cell potentials? If there is an effect, please suggest an explanation. 3. What is the oxidizing agent in the Zn-Mg cell? ELECTROCHEMISTRY: GALVANIC CELLS 143 E15 nter
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