{"id":258,"date":"2017-06-20T20:45:02","date_gmt":"2017-06-20T20:45:02","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/chemistry2labs\/?post_type=chapter&p=258"},"modified":"2017-06-20T21:27:54","modified_gmt":"2017-06-20T21:27:54","slug":"lab-11-worksheet","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/chemistry2labs\/chapter\/lab-11-worksheet\/","title":{"raw":"Lab 11 Worksheet","rendered":"Lab 11 Worksheet"},"content":{"raw":"
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Download the .pdf file of the lab handout\u00a0here<\/a>.<\/div>\r\nExperimental Procedure and Data\r\n\r\n1. Connect the Vernier voltage probe into thee Logger Pro. Turn on the instrument. Start the Logger Pro.\r\n\r\nPart A: Determining the Cell Potential for Redox Couples.\r\n
    \r\n \t
  1. Obtain 10-20 mL of 1 M KNO3 in a 50 mL beaker. Cut 6 pieces of string, each with a length of\u00a0approximately 2-3 cm. Place the pieces of string in the KNO3 solution. You need to completely saturate\u00a0the string prior to use. This will be your salt bridge.<\/li>\r\n \t
  2. Obtain 3 pieces of each metal samples used in this experiment. Sand both sides of the metal samples\u00a0to produce a shiny surface. If the surface is oxidized, it will prevent an accurate measurement from\u00a0being recorded.<\/li>\r\n \t
  3. Make observations about each metal in the data section.<\/li>\r\n \t
  4. Obtain a well-spot plate.<\/li>\r\n \t
  5. See the diagram below for help. Fill the wells in the spot plate with a 1 M solution of the metal nitrate\u00a0indicated. You need each well to be ~ 3\u20444 full. Make observations about each of the solutions in the\u00a0data section.<\/li>\r\n \t
  6. Use forceps to place a piece of string (soaked in your salt solution) as indicated below. Each end of the\u00a0string will be immersed in a different metal solution.<\/li>\r\n \t
  7. Attach one metal to the positive (red) lead of the voltage probe. Attach the other metal to the negative (black) lead of the voltage probe. Place each metal into THE SAME metal solution (the copper metal goes to the copper nitrate solution, the zinc metal should go in the zinc nitrate solution, etc). Wait approximately 5 seconds before\u00a0recording the voltage.<\/li>\r\n \t
  8. If you obtain a negative voltage, reverse which electrode is attached to each metal<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n<\/colgroup>\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n
    \r\n
    \r\n
    \r\n\r\nTrial\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
    		\r\n
    \r\n
    \r\n\r\nWell Row 1\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
    		\r\n
    \r\n
    \r\n\r\nWell Row 2\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n<\/tr>\r\n
    \r\n
    \r\n
    \r\n\r\n1\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
    		\r\n
    \r\n
    \r\n\r\nCu\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
    		\r\n
    \r\n
    \r\n\r\nAl\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n<\/tr>\r\n
    \r\n
    \r\n
    \r\n\r\n2\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
    		\r\n
    \r\n
    \r\n\r\nCu\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
    		\r\n
    \r\n
    \r\n\r\nMg\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n<\/tr>\r\n
    \r\n
    \r\n
    \r\n\r\n3\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
    		\r\n
    \r\n
    \r\n\r\nCu\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
    		\r\n
    \r\n
    \r\n\r\nZn\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n<\/tr>\r\n
    \r\n
    \r\n
    \r\n\r\n4\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
    		\r\n
    \r\n
    \r\n\r\nMg\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
    		\r\n
    \r\n
    \r\n\r\nAl\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n<\/tr>\r\n
    \r\n
    \r\n
    \r\n\r\n5\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
    		\r\n
    \r\n
    \r\n\r\nMg\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
    		\r\n
    \r\n
    \r\n\r\nZn\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n<\/tr>\r\n
    \r\n
    \r\n
    \r\n\r\n6\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
    		\r\n
    \r\n
    \r\n\r\nAl\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
    		\r\n
    \r\n
    \r\n\r\nMg\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/div>\r\n
    \r\n
    \r\n
    \r\n
      \r\n \t
    1. Record the voltages in your data section.<\/li>\r\n \t
    2. Write the correct equation for each redox reaction in the space provided.<\/li>\r\n \t
    3. Dry each of the metal samples and return them to the tray.<\/li>\r\n \t
    4. Dispose of all waste in the CHM 112 Waste container.<\/li>\r\n \t
    5. A short list of relevant published standard reduction potentials is attached below for help in comparingyour experimental data to the theoretical values.<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n<\/colgroup>\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n
      \r\n
      \r\n
      \r\n\r\nReduction Half Reaction\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		\r\n
      \r\n
      \r\n\r\nE0 (V)\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n<\/tr>\r\n
      \r\n
      \r\n
      \r\n\r\nCu2+(aq) + 2e- \u2192 Cu(s)\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		\r\n
      \r\n
      \r\n\r\n+0.340\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n<\/tr>\r\n
      \r\n
      \r\n
      \r\n\r\n2H+(aq) + 2e- \u2192 H2(g)\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		\r\n
      \r\n
      \r\n\r\n0\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n<\/tr>\r\n
      \r\n
      \r\n
      \r\n\r\nFe2+(aq) + 2e- \u2192 Fe(s)\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		\r\n
      \r\n
      \r\n\r\n-0.440\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n<\/tr>\r\n
      \r\n
      \r\n
      \r\n\r\nZn2+ + 2e- \u2192 Zn(s)\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		\r\n
      \r\n
      \r\n\r\n-0.763\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n<\/tr>\r\n
      \r\n
      \r\n
      \r\n\r\nAl3+(aq) + 3e- \u2192 Al(s)\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		\r\n
      \r\n
      \r\n\r\n-1.676\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n<\/tr>\r\n
      \r\n
      \r\n
      \r\n\r\nMg2+(aq) + 2e- \u2192 Mg(s)\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		\r\n
      \r\n
      \r\n\r\n-2.356\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/div>\r\n
      \r\n
      \r\n
      \r\n\r\n \r\n\r\nPre-lab Assignment\/Questions\r\n\r\n<\/div>\r\n<\/div>\r\n
      \r\n
      \r\n\r\nN o t e \u2013 this pre-lab must be finished before you come to lab.\r\n\r\n1.\u00a0In a galvanic cell,\r\n\r\na. Where does reduction occur?\r\n\r\nb. Where does oxidation occurs?\r\n\r\nc. Anions from the salt bridge flow toward the (which electrode)?\r\n\r\nd. Cations from the salt bridge flow toward the (which electrode?\r\n\r\n2. Consider a galvanic cell consisting of\r\nFe2+ + 2e- \u2192 Fe E0red = -0.44 V\r\n\r\nAl3+ + 3e- \u2192 Al E0red = -1.66 V\r\n\r\n<\/div>\r\n<\/div>\r\n
      \r\n
      \r\n\r\na. Write the reaction occurring at the anode:\r\n\r\nb. Write the reaction occurring at the cathode:\r\n\r\nc. Write the reaction for the galvanic cell.\r\n\r\nd. Calculate the E0cell for the cell.\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n
      \r\n
      \r\n
      \r\n\r\nExperimental Data and Results\r\n\r\nPart A: Determining the Cell Potential for Redox Couples.\r\n\r\n<\/div>\r\n<\/div>\r\n<\/colgroup>\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n
      \r\n
      \r\n
      \r\n\r\nGalvanic Cell\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		\r\n
      \r\n
      \r\n\r\nE0cell\r\n\r\nMeasured\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		\r\n
      \r\n
      \r\n\r\nAnode\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		\r\n
      \r\n
      \r\n\r\nAnode Equation\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		\r\n
      \r\n
      \r\n\r\nCathode\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		\r\n
      \r\n
      \r\n\r\nCathode Equation\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		\r\n
      \r\n
      \r\n\r\nBalanced Equation for Cell\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		\r\n
      \r\n
      \r\n\r\nOxidizing Agent\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		\r\n
      \r\n
      \r\n\r\nReducing Agent\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		\r\n
      \r\n
      \r\n\r\nE0cell Theoretical\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		\r\n
      \r\n
      \r\n\r\nE0cell Percent Error\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n<\/tr>\r\n
      \r\n
      \r\n
      \r\n\r\nCu-Al\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/tr>\r\n
      \r\n
      \r\n
      \r\n\r\nCu-Mg\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/tr>\r\n
      \r\n
      \r\n
      \r\n\r\nCu-Zn\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/tr>\r\n
      \r\n
      \r\n
      \r\n\r\nMg-Al\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/tr>\r\n
      \r\n
      \r\n
      \r\n\r\nMg-Zn\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/tr>\r\n
      \r\n
      \r\n
      \r\n\r\nAl-Zn\r\n\r\n<\/div>\r\n<\/div><\/td>\r\n
      		<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n
      \r\n
      \r\n\r\n*Show an example of all calculations\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n
      \r\n
      \r\n
      \r\n\r\n1. Using your data create an activity series based on the reduction potentials you found.\r\n\r\n<\/div>\r\n<\/div>\r\n
      \r\n
      \r\n\r\n2. Does this activity series agree with the published data? If not, give at least two plausible explanations for what may have occurred.\r\n\r\n<\/div>\r\n<\/div>\r\n
      \u00a0Post-Lab Questions<\/div>\r\n<\/div>\r\n
      \r\n
      \r\n
      \u00a0A positive potential is recorded when copper is attached to the positive (red) electrode. Based on this, do you think copper is the cathode or the anode of the cell? Explain your reasoning\/<\/div>\r\n
      \r\n
        \r\n \t
      1. If your string was not saturated with salt solution, would the potential of the cell have been recorded as too high, too low, or unaffected? Explain your reasoning.<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n
        \r\n
        \u00a0In your Cu-Zn cell you could adjust the concentration of Zn2+ and Cu2+ to maximize cell potential. Would you increase or decrease the copper concentration? Would you increase or decrease the zinc concentration? Explain your reasoning for each choice.<\/div>\r\n<\/div>\r\n<\/div>","rendered":"
        \n
        \n
        \n
        Download the .pdf file of the lab handout\u00a0here<\/a>.<\/div>\n

        Experimental Procedure and Data<\/p>\n

        1. Connect the Vernier voltage probe into thee Logger Pro. Turn on the instrument. Start the Logger Pro.<\/p>\n

        Part A: Determining the Cell Potential for Redox Couples.<\/p>\n

          \n
        1. Obtain 10-20 mL of 1 M KNO3 in a 50 mL beaker. Cut 6 pieces of string, each with a length of\u00a0approximately 2-3 cm. Place the pieces of string in the KNO3 solution. You need to completely saturate\u00a0the string prior to use. This will be your salt bridge.<\/li>\n
        2. Obtain 3 pieces of each metal samples used in this experiment. Sand both sides of the metal samples\u00a0to produce a shiny surface. If the surface is oxidized, it will prevent an accurate measurement from\u00a0being recorded.<\/li>\n
        3. Make observations about each metal in the data section.<\/li>\n
        4. Obtain a well-spot plate.<\/li>\n
        5. See the diagram below for help. Fill the wells in the spot plate with a 1 M solution of the metal nitrate\u00a0indicated. You need each well to be ~ 3\u20444 full. Make observations about each of the solutions in the\u00a0data section.<\/li>\n
        6. Use forceps to place a piece of string (soaked in your salt solution) as indicated below. Each end of the\u00a0string will be immersed in a different metal solution.<\/li>\n
        7. Attach one metal to the positive (red) lead of the voltage probe. Attach the other metal to the negative (black) lead of the voltage probe. Place each metal into THE SAME metal solution (the copper metal goes to the copper nitrate solution, the zinc metal should go in the zinc nitrate solution, etc). Wait approximately 5 seconds before\u00a0recording the voltage.<\/li>\n
        8. If you obtain a negative voltage, reverse which electrode is attached to each metal<\/li>\n<\/ol>\n<\/div>\n<\/div>\n\n\n\n\n<\/colgroup>\n\n\n\n\n\n\n\n\n
          \n
          \n
          \n

          Trial<\/p>\n<\/div>\n<\/div>\n<\/td>\n

          		\n
          \n
          \n

          Well Row 1<\/p>\n<\/div>\n<\/div>\n<\/td>\n

          		\n
          \n
          \n

          Well Row 2<\/p>\n<\/div>\n<\/div>\n<\/td>\n<\/tr>\n

          \n
          \n
          \n

          1<\/p>\n<\/div>\n<\/div>\n<\/td>\n

          		\n
          \n
          \n

          Cu<\/p>\n<\/div>\n<\/div>\n<\/td>\n

          		\n
          \n
          \n

          Al<\/p>\n<\/div>\n<\/div>\n<\/td>\n<\/tr>\n

          \n
          \n
          \n

          2<\/p>\n<\/div>\n<\/div>\n<\/td>\n

          		\n
          \n
          \n

          Cu<\/p>\n<\/div>\n<\/div>\n<\/td>\n

          		\n
          \n
          \n

          Mg<\/p>\n<\/div>\n<\/div>\n<\/td>\n<\/tr>\n

          \n
          \n
          \n

          3<\/p>\n<\/div>\n<\/div>\n<\/td>\n

          		\n
          \n
          \n

          Cu<\/p>\n<\/div>\n<\/div>\n<\/td>\n

          		\n
          \n
          \n

          Zn<\/p>\n<\/div>\n<\/div>\n<\/td>\n<\/tr>\n

          \n
          \n
          \n

          4<\/p>\n<\/div>\n<\/div>\n<\/td>\n

          		\n
          \n
          \n

          Mg<\/p>\n<\/div>\n<\/div>\n<\/td>\n

          		\n
          \n
          \n

          Al<\/p>\n<\/div>\n<\/div>\n<\/td>\n<\/tr>\n

          \n
          \n
          \n

          5<\/p>\n<\/div>\n<\/div>\n<\/td>\n

          		\n
          \n
          \n

          Mg<\/p>\n<\/div>\n<\/div>\n<\/td>\n

          		\n
          \n
          \n

          Zn<\/p>\n<\/div>\n<\/div>\n<\/td>\n<\/tr>\n

          \n
          \n
          \n

          6<\/p>\n<\/div>\n<\/div>\n<\/td>\n

          		\n
          \n
          \n

          Al<\/p>\n<\/div>\n<\/div>\n<\/td>\n

          		\n
          \n
          \n

          Mg<\/p>\n<\/div>\n<\/div>\n<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n

          \n
          \n
          \n
            \n
          1. Record the voltages in your data section.<\/li>\n
          2. Write the correct equation for each redox reaction in the space provided.<\/li>\n
          3. Dry each of the metal samples and return them to the tray.<\/li>\n
          4. Dispose of all waste in the CHM 112 Waste container.<\/li>\n
          5. A short list of relevant published standard reduction potentials is attached below for help in comparingyour experimental data to the theoretical values.<\/li>\n<\/ol>\n<\/div>\n<\/div>\n\n\n\n<\/colgroup>\n\n\n\n\n\n\n\n\n
            \n
            \n
            \n

            Reduction Half Reaction<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		\n
            \n
            \n

            E0 (V)<\/p>\n<\/div>\n<\/div>\n<\/td>\n<\/tr>\n

            \n
            \n
            \n

            Cu2+(aq) + 2e- \u2192 Cu(s)<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		\n
            \n
            \n

            +0.340<\/p>\n<\/div>\n<\/div>\n<\/td>\n<\/tr>\n

            \n
            \n
            \n

            2H+(aq) + 2e- \u2192 H2(g)<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		\n
            \n
            \n

            0<\/p>\n<\/div>\n<\/div>\n<\/td>\n<\/tr>\n

            \n
            \n
            \n

            Fe2+(aq) + 2e- \u2192 Fe(s)<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		\n
            \n
            \n

            -0.440<\/p>\n<\/div>\n<\/div>\n<\/td>\n<\/tr>\n

            \n
            \n
            \n

            Zn2+ + 2e- \u2192 Zn(s)<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		\n
            \n
            \n

            -0.763<\/p>\n<\/div>\n<\/div>\n<\/td>\n<\/tr>\n

            \n
            \n
            \n

            Al3+(aq) + 3e- \u2192 Al(s)<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		\n
            \n
            \n

            -1.676<\/p>\n<\/div>\n<\/div>\n<\/td>\n<\/tr>\n

            \n
            \n
            \n

            Mg2+(aq) + 2e- \u2192 Mg(s)<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		\n
            \n
            \n

            -2.356<\/p>\n<\/div>\n<\/div>\n<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n

            \n
            \n
            \n

             <\/p>\n

            Pre-lab Assignment\/Questions<\/p>\n<\/div>\n<\/div>\n

            \n
            \n

            N o t e \u2013 this pre-lab must be finished before you come to lab.<\/p>\n

            1.\u00a0In a galvanic cell,<\/p>\n

            a. Where does reduction occur?<\/p>\n

            b. Where does oxidation occurs?<\/p>\n

            c. Anions from the salt bridge flow toward the (which electrode)?<\/p>\n

            d. Cations from the salt bridge flow toward the (which electrode?<\/p>\n

            2. Consider a galvanic cell consisting of
            \nFe2+ + 2e- \u2192 Fe E0red = -0.44 V<\/p>\n

            Al3+ + 3e- \u2192 Al E0red = -1.66 V<\/p>\n<\/div>\n<\/div>\n

            \n
            \n

            a. Write the reaction occurring at the anode:<\/p>\n

            b. Write the reaction occurring at the cathode:<\/p>\n

            c. Write the reaction for the galvanic cell.<\/p>\n

            d. Calculate the E0cell for the cell.<\/p>\n<\/div>\n<\/div>\n<\/div>\n

            \n
            \n
            \n

            Experimental Data and Results<\/p>\n

            Part A: Determining the Cell Potential for Redox Couples.<\/p>\n<\/div>\n<\/div>\n\n\n\n\n\n\n\n\n\n\n\n\n<\/colgroup>\n\n\n\n\n\n\n\n\n
            \n
            \n
            \n

            Galvanic Cell<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		\n
            \n
            \n

            E0cell<\/p>\n

            Measured<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		\n
            \n
            \n

            Anode<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		\n
            \n
            \n

            Anode Equation<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		\n
            \n
            \n

            Cathode<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		\n
            \n
            \n

            Cathode Equation<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		\n
            \n
            \n

            Balanced Equation for Cell<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		\n
            \n
            \n

            Oxidizing Agent<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		\n
            \n
            \n

            Reducing Agent<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		\n
            \n
            \n

            E0cell Theoretical<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		\n
            \n
            \n

            E0cell Percent Error<\/p>\n<\/div>\n<\/div>\n<\/td>\n<\/tr>\n

            \n
            \n
            \n

            Cu-Al<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/tr>\n
            \n
            \n
            \n

            Cu-Mg<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/tr>\n
            \n
            \n
            \n

            Cu-Zn<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/tr>\n
            \n
            \n
            \n

            Mg-Al<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/tr>\n
            \n
            \n
            \n

            Mg-Zn<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/tr>\n
            \n
            \n
            \n

            Al-Zn<\/p>\n<\/div>\n<\/div>\n<\/td>\n

            		<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n
            \n
            \n

            *Show an example of all calculations<\/p>\n<\/div>\n<\/div>\n<\/div>\n

            \n
            \n
            \n

            1. Using your data create an activity series based on the reduction potentials you found.<\/p>\n<\/div>\n<\/div>\n

            \n
            \n

            2. Does this activity series agree with the published data? If not, give at least two plausible explanations for what may have occurred.<\/p>\n<\/div>\n<\/div>\n

            \u00a0Post-Lab Questions<\/div>\n<\/div>\n
            \n
            \n
            \u00a0A positive potential is recorded when copper is attached to the positive (red) electrode. Based on this, do you think copper is the cathode or the anode of the cell? Explain your reasoning\/<\/div>\n
            \n
              \n
            1. If your string was not saturated with salt solution, would the potential of the cell have been recorded as too high, too low, or unaffected? Explain your reasoning.<\/li>\n<\/ol>\n<\/div>\n<\/div>\n
              \n
              \u00a0In your Cu-Zn cell you could adjust the concentration of Zn2+ and Cu2+ to maximize cell potential. Would you increase or decrease the copper concentration? Would you increase or decrease the zinc concentration? Explain your reasoning for each choice.<\/div>\n<\/div>\n<\/div>\n","protected":false},"author":23588,"menu_order":4,"template":"","meta":{"_candela_citation":"[]","CANDELA_OUTCOMES_GUID":"","pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-258","chapter","type-chapter","status-publish","hentry"],"part":29,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/chemistry2labs\/wp-json\/pressbooks\/v2\/chapters\/258","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/courses.lumenlearning.com\/chemistry2labs\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/courses.lumenlearning.com\/chemistry2labs\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/chemistry2labs\/wp-json\/wp\/v2\/users\/23588"}],"version-history":[{"count":3,"href":"https:\/\/courses.lumenlearning.com\/chemistry2labs\/wp-json\/pressbooks\/v2\/chapters\/258\/revisions"}],"predecessor-version":[{"id":302,"href":"https:\/\/courses.lumenlearning.com\/chemistry2labs\/wp-json\/pressbooks\/v2\/chapters\/258\/revisions\/302"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/chemistry2labs\/wp-json\/pressbooks\/v2\/parts\/29"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/chemistry2labs\/wp-json\/pressbooks\/v2\/chapters\/258\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/chemistry2labs\/wp-json\/wp\/v2\/media?parent=258"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/chemistry2labs\/wp-json\/pressbooks\/v2\/chapter-type?post=258"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/chemistry2labs\/wp-json\/wp\/v2\/contributor?post=258"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/chemistry2labs\/wp-json\/wp\/v2\/license?post=258"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}