Reference no: EM132743858 , Length: 1275 Words
Experiment - GALVANIC CELLS
Part A. Activity Series
Create a new table similar in structure to your data table for Part A of the lab. Include in your table which species was reduced and which was oxidized.
1. Underneath the table, give the ranking of the metals from strongest reducing agent to weakest reducing agent based on your observations. Explain your rankings.
Part B. Galvanic Cells
Create a table like the following example and fill in the cell-line notation description of the cell (remember, oxidation is always first, then reduction), the balanced redox reaction occurring, and the potential of each.
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Cell-Line Notation
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Reaction
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Potential
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2. Which lead is connected to the half-cell undergoing oxidation? Which lead is connected to the half-cell undergoing reduction?
3. Do these reactions follow the same trend of reducing power you found in part A?
4. Do the potentials of these three reactions support that potential is a state function? Why or why not? (Hint: This is like a Hess's law problem - can you add together 2 of the reactions to get the third reaction? Do the potentials add in the same way?)
5. If the reduction potential of the zinc half-reaction is set to 0V, then what is the reduction potential of the copper half-reaction? Of the silver half-reaction?
6. If the reduction potential of the copper half-reaction is set to 0V, then what is the reduction potential of the zinc half-reaction? Of the silver half-reaction?
7. If the reduction potential of the silver half-reaction is set to 2V, then what is the reduction potential of the copper half-reaction? Of the zinc-half reaction?
Part C. Nonstandard Galvanic Cells
Create a table like the one in part B and fill in the cell-line notation for the cell (including concentrations since they are nonstandard!), the balanced redox reaction occurring, and the potential of each.
8. Is the potential of the zinc and copper cell with 0.1M concentrations the same as or different from the standard potential of the cell? Explain why this is the case.
9. Is the potential of the zinc and silver cell with 0.1M concentrations the same as or different from the standard potential of the cell? Explain why this is the case.
10. Show how to calculate the potential of the 2M Zn 0.001M Cu cell using the Nernst equation. DON'T FORGET TO USE EQUATION EDITOR. Nonformatted answers will not be graded.
Part D. Concentration Cells
Create a table like the ones in parts B and C and fill in the cell-line notation for the cell (including concentrations for the nonstandard cell), the balanced redox reaction occurring (include subscripts of "an" for the anode components and "cat" for the cathode components), and the potential of both cells.
11. Explain why the potential of the standard copper/copper cell makes sense.
12. Explain why the potential of the nonstandard copper/copper cell makes sense. Which concentration half-cell is the anode? Which concentration half-cell is the cathode?
13. Calculate the potential of the nonstandard copper/copper cell using the Nernst equation. DON'T FORGET TO USE EQUATION EDITOR. Nonformatted answers will not be graded.
Attachment:- GALVANIC CELLS.rar