CHEM1010H - Electrochemistry and the Nernst Equation Assignment

Assignment Task

Part

A. Investigating the Transfer of Electrons Via the Reactivity of Metals in Solutions

1. Based on your observations of each metal/solution pair, indicate which metal is the anode and which is the cathode in each reaction. Click the appropriate box for each column.

2. Using Zinc and Copper as an example, show the complete half-cell reactions for the redox reaction between these two metals, and then give the cell notation for an electrochemical cell using these two metals as electrodes. Note: You will need to complete these equations in another program (such as equation editor in MS Word) and then insert as an image below.

B. Preparing Electrolyte Solution and the Electrochemical Half-Cell.

3. Calculate the exact concentration of your KNO3 solution. Show the complete calculation. You will need to insert your calculation as an image below.

C. Identification of Unknown Metal/Metal Solutions using Ecell Measurements

4. Calculate the standard cell potential, Eo cell, for each of the possible pairs of metals. Show one complete sample calculation (using one pair of metals) then complete Table 4.

5. Based on your observations of the reactivity in Part A and the voltage readings obtained from Part B for each pair of metals, place each unknown metal in the correct order with respect to the electrochemical series with the strongest oxidizing agents at the top of the list and the strongest reducing agents at the bottom

6. Compare your list of reactivities and theoretical Ecell values to identify each of the unknown metals

7. Measured cell potentials are often different from theoretical values. Compare the measured potential to the theoretical values and calculate the percent error for each pair of metals (using your previous identification). Show one complete sample error calculation (using one pair of metals) then complete Table 5. You will need to insert your calculation as an image below

D. Cu2+ Concentration and the Nernst Equation

8. Calculate the concentration of Cu2+ in each diluted CuSO4 solution. Show one complete sample calculation, then tabulate the other solutions (Table 5). Insert your calculation as an image.

9. How does the concentration of the solutions affect the measured voltage?

10. Use the Nernst equation to calculate the theoretical Ecell value for the “stock” solution of Cu2+ with a 0.50M Zn2+ solution.

11. Construct a Nernst plot of Ecell vs ln[Cu2+], from Table 6. Your plot should include a line of best fit, the equation the line (with the y-intercept and slope) and best fit (R2 ) values to 3 decimal places. You are encouraged to use an appropriate graphing program to complete the plot electronically. Graphs should follow the graphing format provided in the Student Laboratory Handbook. You will need to save your graph as an image then insert into the box below.

12. Using the equation of the line from your Nernst plot, calculate the concentration of a Cu2+ solution that gives a Ecell reading of 1.02V.

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