Homework Help is Here – Start Your Trial Now!
Science
Chemistry
1. Write the RHR, OHR, and the balanced overall reaction of the voltaic cell. 2. Prove that the reaction in the voltaic cell is spontaneous by calculating E°cel using Eqn 11b-1 and the values listed in Table S1 of the Supplementary Material. 3. Calculate the theoretical Ecel using the Nernst Equation (Eqn 11b-2). 4. Compare the experimental Ecel from Table 11b-1 to the theoretical Ecel by calculating percent error using Eqn 11b- 4. experimental value - literature value % error = x 100 (Eqn 11b-4) literature value

1. Write the RHR, OHR, and the balanced overall reaction of the voltaic cell. 2. Prove that the reaction in the voltaic cell is spontaneous by calculating E°cel using Eqn 11b-1 and the values listed in Table S1 of the Supplementary Material. 3. Calculate the theoretical Ecel using the Nernst Equation (Eqn 11b-2). 4. Compare the experimental Ecel from Table 11b-1 to the theoretical Ecel by calculating percent error using Eqn 11b- 4. experimental value - literature value % error = x 100 (Eqn 11b-4) literature value

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 135CWP: Consider a galvanic cell based on the following half-reactions: a. What is the expected cell...
See similar textbooks
icon
Related questions
Question
100%
1. Voltaic Cell For this part, refer to the following: Setup 2 Anode Setup 1 Setup 3 Anode Cathode Cathode Anode Cathode Electrodes Zinc Silver Zinc Silver Zinc Silver AGNO3(aqg) 0.10 M Zn(NO3)2 0.10 M Solutions Zn(NO3)2 1.0 M AGNO3(aq) 1.0 M Zn(NO:)2 1.0 M AGNO3 1.0 M Concentrations Following Setup 1, place 50.0 mL each of 1.0 M Zn(NO3)2 and 1.0 M AGNO3 solutions in two separate 100-mL beakers. Dip a Zn electrode into the Zn(NO3)2 solution and an Ag electrode into the AGNO3 solution, and connect the two solutions by a salt bridge containing saturated KNO3. Make sure that one end of the salt bridge dips into the Zn(NO3)2 solution and the other into the AGNO3 solution. Connect the Zn electrode to the negative terminal of the voltmeter and the Ag electrode to the positive terminal. Allow the cell to stand for five minutes and read the cell potential and the Repeat the procedure following Setups 2 and 3. saton Division, Institue For a simple demonstration of this experiment, watch this short video: https://www.youtube.com/watch?v=DafEX2FD4Ado. Note that the electrodes and electrolyte solutions used in the demonstration are different from the ones enumerated in the Setups above. Pay attention to how the voltaic cell is put together from its components. nuna.
Transcribed Image Text:1. Voltaic Cell For this part, refer to the following: Setup 2 Anode Setup 1 Setup 3 Anode Cathode Cathode Anode Cathode Electrodes Zinc Silver Zinc Silver Zinc Silver AGNO3(aqg) 0.10 M Zn(NO3)2 0.10 M Solutions Zn(NO3)2 1.0 M AGNO3(aq) 1.0 M Zn(NO:)2 1.0 M AGNO3 1.0 M Concentrations Following Setup 1, place 50.0 mL each of 1.0 M Zn(NO3)2 and 1.0 M AGNO3 solutions in two separate 100-mL beakers. Dip a Zn electrode into the Zn(NO3)2 solution and an Ag electrode into the AGNO3 solution, and connect the two solutions by a salt bridge containing saturated KNO3. Make sure that one end of the salt bridge dips into the Zn(NO3)2 solution and the other into the AGNO3 solution. Connect the Zn electrode to the negative terminal of the voltmeter and the Ag electrode to the positive terminal. Allow the cell to stand for five minutes and read the cell potential and the Repeat the procedure following Setups 2 and 3. saton Division, Institue For a simple demonstration of this experiment, watch this short video: https://www.youtube.com/watch?v=DafEX2FD4Ado. Note that the electrodes and electrolyte solutions used in the demonstration are different from the ones enumerated in the Setups above. Pay attention to how the voltaic cell is put together from its components. nuna.
A. VOLTAIC CELL 1. Write the RHR, OHR, and the balanced overall reaction of the voltaic cell. Prove that the reaction in the voltaic cell is spontaneous by calculating E°cell using Egn 11b-1 and the values listed in Table S1 of the Supplementary Material. 3. Calculate the theoretical Ecell using the Nernst Equation (Eqn 11b-2). 4. Compare the experimental Ecell from Table 11b-1 to the theoretical Ecell by calculating percent error using Egn 11b- 4. 2. experimental value - literature value % error = x 100 (Eqn 11b-4) literature value Note: Steps 3 and 4 should be done for EACH setup.
Transcribed Image Text:A. VOLTAIC CELL 1. Write the RHR, OHR, and the balanced overall reaction of the voltaic cell. Prove that the reaction in the voltaic cell is spontaneous by calculating E°cell using Egn 11b-1 and the values listed in Table S1 of the Supplementary Material. 3. Calculate the theoretical Ecell using the Nernst Equation (Eqn 11b-2). 4. Compare the experimental Ecell from Table 11b-1 to the theoretical Ecell by calculating percent error using Egn 11b- 4. 2. experimental value - literature value % error = x 100 (Eqn 11b-4) literature value Note: Steps 3 and 4 should be done for EACH setup.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps with 3 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Follow-up Questions
Read through expert solutions to related follow-up questions below.
Follow-up Question

Solutions and Answers from numbers 2-3

A. VOLTAIC CELL 1. Write the RHR, OHR, and the balanced overall reaction of the voltaic cell. 2. Prove that the reaction in the voltaic cell is spontaneous by calculating Eºcell using Eqn 11b-1 and the values listed in Table S1 of the Supplementary Material. 3. Calculate the theoretical Ecell using the Nernst Equation (Eqn 11b-2). 4. Compare the experimental Ecell from Table 11b-1 to the theoretical Ecell by calculating percent error using Eqn 11b- 4. % error = experimental value - literature value literature value x 100 (Eqn 11b-4) Note: Steps 3 and 4 should be done for EACH setup.
Transcribed Image Text:A. VOLTAIC CELL 1. Write the RHR, OHR, and the balanced overall reaction of the voltaic cell. 2. Prove that the reaction in the voltaic cell is spontaneous by calculating Eºcell using Eqn 11b-1 and the values listed in Table S1 of the Supplementary Material. 3. Calculate the theoretical Ecell using the Nernst Equation (Eqn 11b-2). 4. Compare the experimental Ecell from Table 11b-1 to the theoretical Ecell by calculating percent error using Eqn 11b- 4. % error = experimental value - literature value literature value x 100 (Eqn 11b-4) Note: Steps 3 and 4 should be done for EACH setup.
1. Voltaic Cell For this part, refer to the following: Anode Anode Electrodes Anode Zinc Zn(NO3)2 Cathode Silver AgNO3(aq) Cathode Silver Solutions Concentrations Cathode Silver AgNO3(aq) 0.10 M Zinc Zn(NO3)2 1.0 M Zinc Zn(NO3)2 AgNO3 1.0 M 1.0 M 0.10 M 1.0 M Following Setup 1, place 50.0 mL each of 1.0 M Zn(NO3)2 and 1.0 M AgNO3 solutions in two separate 100-mL beakers. Dip a Zn electrode into the Zn(NO3)2 solution and an Ag electrode into the AgNO3 solution, and connect the two solutions by a salt bridge containing saturated KNO3. Make sure that one end of the salt bridge dips into the Zn(NO3)2 solution and the other into the AgNO3 solution. Connect the Zn electrode to the negative terminal of the voltmeter and the Ag electrode to the positive terminal. Allow the cell to stand for five minutes and read the cell potential and the the solutions. Repeat the described procedure following Setups 2 and Step 2 ted without the written temperature of Division, For a simple demonstration of this experiment, watch this short video: https://www.youtube.com/watch?v=afEX2FD4Ado. Note that the electrodes and electrolyte solutions used in the demonstration are different from the ones enumerated in the Setups above. Pay attention to how the voltaic cell is put together from its components. to how the voltaic cell is put toget Setup 1 Setup 2 Setup 3
Transcribed Image Text:1. Voltaic Cell For this part, refer to the following: Anode Anode Electrodes Anode Zinc Zn(NO3)2 Cathode Silver AgNO3(aq) Cathode Silver Solutions Concentrations Cathode Silver AgNO3(aq) 0.10 M Zinc Zn(NO3)2 1.0 M Zinc Zn(NO3)2 AgNO3 1.0 M 1.0 M 0.10 M 1.0 M Following Setup 1, place 50.0 mL each of 1.0 M Zn(NO3)2 and 1.0 M AgNO3 solutions in two separate 100-mL beakers. Dip a Zn electrode into the Zn(NO3)2 solution and an Ag electrode into the AgNO3 solution, and connect the two solutions by a salt bridge containing saturated KNO3. Make sure that one end of the salt bridge dips into the Zn(NO3)2 solution and the other into the AgNO3 solution. Connect the Zn electrode to the negative terminal of the voltmeter and the Ag electrode to the positive terminal. Allow the cell to stand for five minutes and read the cell potential and the the solutions. Repeat the described procedure following Setups 2 and Step 2 ted without the written temperature of Division, For a simple demonstration of this experiment, watch this short video: https://www.youtube.com/watch?v=afEX2FD4Ado. Note that the electrodes and electrolyte solutions used in the demonstration are different from the ones enumerated in the Setups above. Pay attention to how the voltaic cell is put together from its components. to how the voltaic cell is put toget Setup 1 Setup 2 Setup 3
Solution
Bartleby Expert
SEE SOLUTION
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
Recommended textbooks for you
Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781133611097
Author:
Steven S. Zumdahl
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry: Principles and Practice
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
Chemistry for Engineering Students
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
SEE MORE TEXTBOOKS