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3. Determine the equilibrium constant for the zinc and copper battery.

3. Determine the equilibrium constant for the zinc and copper battery.

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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Lab #21-Electrochemical Cells red=inpert black = common Objective: I will measure the potential difference of dissimilar metals. Background: Materials: ♦ . . . . Voltmeter Coffee Filter Vinegar Zinc Zn Iron Pb Cu red *** Cu black Pb black 558.5 Sn black 566.9 Zn black Al black Mg black 1.002 0.662 1.741 Procedure: 1. Flatten the coffee filter on your lab desk, and dampen it completely with vinegar. 2. Place the 6 metal samples evenly spaced on the outside edge of the coffee filter. 3. Set the voltmeter to DC volts. 4. Firmly press the positive and negative electrodes into the metals. 5. Record the voltage in the data table. Note: The voltage will drop over time. Record the highest voltage that you see. 6. Reverse the electrodes, and record the voltage in the data table. 7. Determine and record the potential differences of all other combinations of metals. Data Collection: 36.8 -430.2 -81.3 -1,156 . . - . 463.8 113.1 1.196 Zine Erd=-0.76 V Copper | Ered = +0.34 V . Measured Potential Difference Pb red Sn red Zn red |-5456-530.2 -1.009 220229 37.9 -444.9 -465,6 Magnesium Tin n Aluminum A Copper Cu -361,7 Al red Mg red -0,642 -1.707 -74.2 -1.143 -99,11. 171 370.9 -0.69 0.708 | 1,048 -1.659 Conclusion Questions: 1. A battery is made using zinc and copper. Determine and label the balanced oxidation and reduction half-reactions. 2. The accepted standard reduction potentials for copper and zinc are listed below. What is the accepted value for the Fell? C
Transcribed Image Text:Lab #21-Electrochemical Cells red=inpert black = common Objective: I will measure the potential difference of dissimilar metals. Background: Materials: ♦ . . . . Voltmeter Coffee Filter Vinegar Zinc Zn Iron Pb Cu red *** Cu black Pb black 558.5 Sn black 566.9 Zn black Al black Mg black 1.002 0.662 1.741 Procedure: 1. Flatten the coffee filter on your lab desk, and dampen it completely with vinegar. 2. Place the 6 metal samples evenly spaced on the outside edge of the coffee filter. 3. Set the voltmeter to DC volts. 4. Firmly press the positive and negative electrodes into the metals. 5. Record the voltage in the data table. Note: The voltage will drop over time. Record the highest voltage that you see. 6. Reverse the electrodes, and record the voltage in the data table. 7. Determine and record the potential differences of all other combinations of metals. Data Collection: 36.8 -430.2 -81.3 -1,156 . . - . 463.8 113.1 1.196 Zine Erd=-0.76 V Copper | Ered = +0.34 V . Measured Potential Difference Pb red Sn red Zn red |-5456-530.2 -1.009 220229 37.9 -444.9 -465,6 Magnesium Tin n Aluminum A Copper Cu -361,7 Al red Mg red -0,642 -1.707 -74.2 -1.143 -99,11. 171 370.9 -0.69 0.708 | 1,048 -1.659 Conclusion Questions: 1. A battery is made using zinc and copper. Determine and label the balanced oxidation and reduction half-reactions. 2. The accepted standard reduction potentials for copper and zinc are listed below. What is the accepted value for the Fell? C
AP Chemistry Lab # 21- Electrochemical Cells 3. Determine the equilibrium constant for the zinc and copper battery. 4. A battery is made from the metals with the greatest potential difference. On the diagram below, label the: a. Metal electrodes b. Oxidation and reduction sides C. Anode and cathode d. Direction of electron flow
Transcribed Image Text:AP Chemistry Lab # 21- Electrochemical Cells 3. Determine the equilibrium constant for the zinc and copper battery. 4. A battery is made from the metals with the greatest potential difference. On the diagram below, label the: a. Metal electrodes b. Oxidation and reduction sides C. Anode and cathode d. Direction of electron flow
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