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Experiment #10 Worksheet Name: Table A. Lead/Copper Redox System Experimental Observations Oxidation Half-Rxn E°rod anode)= Reduction Half-Rxn EOd cathode)=

Experiment #10 Worksheet Name: Table A. Lead/Copper Redox System Experimental Observations Oxidation Half-Rxn E°rod anode)= Reduction Half-Rxn EOd cathode)=

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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PROCEDURE Qualitative Analysis of Electrochemical Cells In this portion of the experiment you will be looking at the spontaneous redox reaction of three different metals with copper(II) nitrate, Cu(NO3)2. A. Lead (Pb) and Copper (Cu) Redox System Take a lead (Pb) strip and, using sandpaper, lightly sand until the metal is shiny. (Be sure to collect the sandings and dispose them in the waste container) Place the lead strip into a small test tube or 50 mL beaker and add enough 0.5 M Cu(NO3)2 solution to cover the bottom of the strip (about 2 cm). Watch the reaction and after 2.5 minutes record your observations in Table A. Allow the reaction to progress another 2.5 minutes and record your observations in 1. 2. 3. 4. Table A. 5. Remove the lead strip, rinse it with distilled water and dry with a paper towel. Clean off and discard any newly formed material with sandpaper or steel wool and keep the metal for part D. Keep the Cu(NO3)2 for use in part B. 6. B. Zinc (Zn) and Copper (Cu) Redox System 1. Take a zinc (Zn) strip and, using sandpaper, lightly sand until the metal is shiny. (Be sure to collect the sandings and dispose them in the waste container) Place the zinc strip into your 0.5 M Cu(NO3)2 solution from part A. Watch the reaction and after 2.5 minutes record your observations in Table B. Allow the reaction to progress another 2.5 minutes and record your observations in Table B. 2. 3. 4. Remove the zinc strip, rinse it with distilled water and dry with a paper towel. Clean off and discard any newly formed material with sandpaper or steel wool and keep the metal for part D. Discard the Cu(NO:)2 solution in the waste jug. 5. 6. C. Zinc (Zn) and Lead (Pb) Redox System 1. Take a zinc (Zn) strip and, using sandpaper, lightly sand until the metal is shiny. (Be sure to collect the sandings and dispose them in the waste container) Place the zinc strip into 20 mL of a 0.5 M Pb(NO3)2 solution. Watch the reaction and after 2.5 minutes record your observations in Table C. Allow the reaction to progress another 2.5 minutes and record your observations in Table C. 2. 3. 4. 5. Remove the zinc strip, rinse it with distilled water and dry with a paper towel. Clean off and discard any newly formed material with sand paper or steel wool and keep the metal for part D. Discard the Pb(NO:)2 solution in the waste jug. 6.
Transcribed Image Text:PROCEDURE Qualitative Analysis of Electrochemical Cells In this portion of the experiment you will be looking at the spontaneous redox reaction of three different metals with copper(II) nitrate, Cu(NO3)2. A. Lead (Pb) and Copper (Cu) Redox System Take a lead (Pb) strip and, using sandpaper, lightly sand until the metal is shiny. (Be sure to collect the sandings and dispose them in the waste container) Place the lead strip into a small test tube or 50 mL beaker and add enough 0.5 M Cu(NO3)2 solution to cover the bottom of the strip (about 2 cm). Watch the reaction and after 2.5 minutes record your observations in Table A. Allow the reaction to progress another 2.5 minutes and record your observations in 1. 2. 3. 4. Table A. 5. Remove the lead strip, rinse it with distilled water and dry with a paper towel. Clean off and discard any newly formed material with sandpaper or steel wool and keep the metal for part D. Keep the Cu(NO3)2 for use in part B. 6. B. Zinc (Zn) and Copper (Cu) Redox System 1. Take a zinc (Zn) strip and, using sandpaper, lightly sand until the metal is shiny. (Be sure to collect the sandings and dispose them in the waste container) Place the zinc strip into your 0.5 M Cu(NO3)2 solution from part A. Watch the reaction and after 2.5 minutes record your observations in Table B. Allow the reaction to progress another 2.5 minutes and record your observations in Table B. 2. 3. 4. Remove the zinc strip, rinse it with distilled water and dry with a paper towel. Clean off and discard any newly formed material with sandpaper or steel wool and keep the metal for part D. Discard the Cu(NO:)2 solution in the waste jug. 5. 6. C. Zinc (Zn) and Lead (Pb) Redox System 1. Take a zinc (Zn) strip and, using sandpaper, lightly sand until the metal is shiny. (Be sure to collect the sandings and dispose them in the waste container) Place the zinc strip into 20 mL of a 0.5 M Pb(NO3)2 solution. Watch the reaction and after 2.5 minutes record your observations in Table C. Allow the reaction to progress another 2.5 minutes and record your observations in Table C. 2. 3. 4. 5. Remove the zinc strip, rinse it with distilled water and dry with a paper towel. Clean off and discard any newly formed material with sand paper or steel wool and keep the metal for part D. Discard the Pb(NO:)2 solution in the waste jug. 6.
Experiment #10 Worksheet Name: Table A. Lead/Copper Redox System Experimental Observations Oxidation Half-Rxn E°rod( anode)= Reduction Half-Rxn E°rod( cathode)= Net Rxn E(cell)= Calculations: Table B. Zinc/Copper Redox System Experimental Observations Oxidation Half-Rxn E°rod( anode)= Reduction Half-Rxn E°rod cathode)= Net Rxn E(cell)= Calculations: Table C. Zinc/Lead Redox System Experimental Observations Oxidation Half-Rxn E°nd(anode)= Reduction Half-Rxn E° rd(cathode)= Net Rxn E°(cell)= Calculations:
Transcribed Image Text:Experiment #10 Worksheet Name: Table A. Lead/Copper Redox System Experimental Observations Oxidation Half-Rxn E°rod( anode)= Reduction Half-Rxn E°rod( cathode)= Net Rxn E(cell)= Calculations: Table B. Zinc/Copper Redox System Experimental Observations Oxidation Half-Rxn E°rod( anode)= Reduction Half-Rxn E°rod cathode)= Net Rxn E(cell)= Calculations: Table C. Zinc/Lead Redox System Experimental Observations Oxidation Half-Rxn E°nd(anode)= Reduction Half-Rxn E° rd(cathode)= Net Rxn E°(cell)= Calculations:
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