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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
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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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.
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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
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