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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. Electrodes Zn Cu Zn Cu Zn Cu Zn Mg Conc. of Each Cation 1.0 M Zn²+ 0.5 M Cu²+ 1.0 M Zn²+ Half-Reactions A. Determine the E for the Standard Zn-Cu Galvanic Cell +2e-Zn -0.76 V Zn²+ (aq) 0.1 M Cu²+ 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 Zn²+ + 2e → Zn (aq) Cu²+2e-Cu (aq) Zn²+ (aq) 1 +2e-Zn Cathode or Anode? Cu²+ + 2e-Cu (aq) Anode - E₁ E E cell cell (table) (cale'd) (measured) +0.34 V 0.46V Cathode 0.34 v anode 0.76v Cathode 0.34 v C. Determine the E for Zn-Mg and Cu-Mg Galvanic Cells 24 1.0 M Zn²+ Zn(aq) + 2€ Zn (s) Cathode -0.76v - 24 1.0 M Mg²+Mga+2e Mg (s) anode -2.38 +1.10V +1.06 v 1.10 1.04 V V 101 0.98 v 10 v1.54 v

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. Electrodes Zn Cu Zn Cu Zn Cu Zn Mg Conc. of Each Cation 1.0 M Zn²+ 0.5 M Cu²+ 1.0 M Zn²+ Half-Reactions A. Determine the E for the Standard Zn-Cu Galvanic Cell +2e-Zn -0.76 V Zn²+ (aq) 0.1 M Cu²+ 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 Zn²+ + 2e → Zn (aq) Cu²+2e-Cu (aq) Zn²+ (aq) 1 +2e-Zn Cathode or Anode? Cu²+ + 2e-Cu (aq) Anode - E₁ E E cell cell (table) (cale'd) (measured) +0.34 V 0.46V Cathode 0.34 v anode 0.76v Cathode 0.34 v C. Determine the E for Zn-Mg and Cu-Mg Galvanic Cells 24 1.0 M Zn²+ Zn(aq) + 2€ Zn (s) Cathode -0.76v - 24 1.0 M Mg²+Mga+2e Mg (s) anode -2.38 +1.10V +1.06 v 1.10 1.04 V V 101 0.98 v 10 v1.54 v

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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what are the E cell cal'cd? Blanks spaces
Name. EXPERIMENT 12 ELECTROCHEMISTRY: GALVANIC CELLS Electrodes Zn 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 Cu Zn Cu Zn Mg Cu Conc. of Each Cation Mg 1.0 M Zn²+ 0.5 M Cu²+ 1.0 M Zn²+ Date 0.1 M Cu²+ Instructor Half-Reactions A. Determine the E for the Standard Zn-Cu Galvanic Cell Zn²+ (aq) + 2e-Zn) -0.76 V Cu²+ + 2e-Cu 1.0 M Cu²+ Cu²+ +2e-Cu Cathode (aq) B. Determine the E* for the Cu-Zn Cell at Non-standard Concentrations 1.0 M Zn²+ 0.46 V Zn²+ + 2e → Zn Anode Zn²+ + 2e → Zn (aq) Cu²+ Cathode or Anode? Report Sheet 1.0 M Zn²+ Zn (aq) +Ze-Zn (s) 1.0 M Mg²+Mga+2e-Mg (s) 1.0 M Cu²+C+Ze Cu(s) - Mg(s) Anode E E (table) (cale) Cathode 0.34 v anode 0.76v cathode 0.34 v (aq) + 2e - Cu C. Determine the E for Zn-Mg and Cu-Mg Galvanic Cells Cathode -0.76 anode -2.38v Cathode 0.34v anode -2.38 +0.34 V +1.10 V +1.06 v 1.10 1.04 V EⓇ (measured) 101 0.98 v 02v 1.54 v 2.72 2+ 1.0 M Mg²+ M +2e "You must use the Nernst equation to calculate this Ecell voltage. (See Equation 8.) CELLS 143 1.98 v ELECTROCHEMISTRY: GALVANIC CELLS 141
Transcribed Image Text:Name. EXPERIMENT 12 ELECTROCHEMISTRY: GALVANIC CELLS Electrodes Zn 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 Cu Zn Cu Zn Mg Cu Conc. of Each Cation Mg 1.0 M Zn²+ 0.5 M Cu²+ 1.0 M Zn²+ Date 0.1 M Cu²+ Instructor Half-Reactions A. Determine the E for the Standard Zn-Cu Galvanic Cell Zn²+ (aq) + 2e-Zn) -0.76 V Cu²+ + 2e-Cu 1.0 M Cu²+ Cu²+ +2e-Cu Cathode (aq) B. Determine the E* for the Cu-Zn Cell at Non-standard Concentrations 1.0 M Zn²+ 0.46 V Zn²+ + 2e → Zn Anode Zn²+ + 2e → Zn (aq) Cu²+ Cathode or Anode? Report Sheet 1.0 M Zn²+ Zn (aq) +Ze-Zn (s) 1.0 M Mg²+Mga+2e-Mg (s) 1.0 M Cu²+C+Ze Cu(s) - Mg(s) Anode E E (table) (cale) Cathode 0.34 v anode 0.76v cathode 0.34 v (aq) + 2e - Cu C. Determine the E for Zn-Mg and Cu-Mg Galvanic Cells Cathode -0.76 anode -2.38v Cathode 0.34v anode -2.38 +0.34 V +1.10 V +1.06 v 1.10 1.04 V EⓇ (measured) 101 0.98 v 02v 1.54 v 2.72 2+ 1.0 M Mg²+ M +2e "You must use the Nernst equation to calculate this Ecell voltage. (See Equation 8.) CELLS 143 1.98 v ELECTROCHEMISTRY: GALVANIC CELLS 141
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