Observations
https://youtu.be/DT3cOf1XDz0 Cell 1
Zn(s) │Zn2+(aq) ║ Cu2+(aq) │Cu(s)
Anode
Cathode
Reduction Half Rxn
Oxidation Half Rxn
Net Cell Rxn
Predicted Standard Cell Potential
Observed Cell Potential
Cell 2
Zn(s) │Zn2+(aq) ║ Fe2+(aq) │Fe(s)
Anode
Cathode
Reduction Half Rxn
Oxidation Half Rxn
Net Cell Rxn
Predicted Standard Cell Potential
Observed Cell Potential
Cell 3
Fe(s) │Fe2+(aq) ║ Cu2+(aq) │Cu(s)
Anode
Cathode
Reduction Half Rxn
Oxidation Half Rxn
Net Cell Rxn
Predicted Standard Cell Potential
Observed Cell Potential
Cell 4
Mg(s) │Mg2+(aq) ║ Zn2+(aq) │Zn(s)
Anode
Cathode
Reduction Half Rxn
Oxidation Half Rxn
Net Cell Rxn
Predicted Standard Cell Potential
Observed Cell Potential
Cell 6
Mg(s) │Mg2+(aq) ║ Cu2+(aq) │Cu(s)
Anode
Cathode
Reduction Half Rxn
Oxidation Half Rxn
Net Cell Rxn
Predicted Standard Cell Potential
Observed Cell Potential
Cell 5
Mg(s) │Mg2+(aq) ║ Fe2+(aq) │Fe(s)
Anode
Cathode
Reduction Half Rxn
Oxidation Half Rxn
Net Cell Rxn
Predicted Standard Cell Potential
Observed Cell Potential
1. Choose two cells from the virtual lab and hand draw a diagram of each cell. Your cell should include two beakers, a salt bridge, wire, voltmeter, anode and cathode. Images cut and paste from the internet will not be graded.
Label the Anode and Cathode
Include the direction of electron movement
Include direction of cations and anions
Cell ____:
Cell ____:
2. Compare the predicted standard cell potentials with the observed values. Was there a discrepancy? Provide possible reasons for any differences.
3. Suggest a reason why very small voltaic cells were constructed for this investigation.
4. Would you expect a difference in the cell potential had larger cells been constructed and tested? Suggest an aspect of a cell’s function that may be affected by using a larger cell that contains a greater quantity of chemicals.
5. A Ni-Cd rechargeable cell has a cell potential of +1.30V. If the cathode has a potential of +0.49 V, what is the anode’s potential?
https://youtu.be/DT3cOf1XDz0