Homework Help is Here – Start Your Trial Now!
Science
Chemistry
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...
See similar textbooks
icon
Related questions
Question
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
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 3 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Electrochemical Cells
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS