Answer Happy

Results Part 1 and 2
Cu/Pb
X/Pb
Y/Pb
Average cell potential (V)
0.4767 V
1.06 V
0.410 V
Results Part 3
Cu concentration
Pb/PbI2
Average cell potential (V)
0.0379 V
0.021 V
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DATA ANALYSIS 1. (Part I) Compare the average cell potential, for your Cu/Pb cell, with the E cell that you calculated in the pre-lab exercise. Explain why your cell potential is different from the text value. 2. (Part II) The unknown metals X and Y were either magnesium, silver, or zinc. Use the text value for the reduction potential of Pb and the measured cell potentials for the unknowns to identify X and Y. 3. (Part III) Use the Nernst equation to calculate the theoretical value of E of the copper- concentration cell and compare this value with the cell potential that you measured. 4. (Part III) Use the Nernst equation and the information that you collected about the Pb/PbI2 cell to complete the following calculations. a. Use the cell potential for the Pb-PbI₂ cell and the known [Pb²+] to calculate the [Pb²+] in equilibrium with PbI2. b. Use the original diluted [Pb²+] and to calculate the in solution. c. Use your data to calculate the Ksp of PbI2 d. The accepted value of the Ksp of PbI2 is 9.8 × 10-º. How does your experimental Ksp of PbI₂ compare with the accepted value?
Electrodes Zn Cu Cu Pb Pb Ag Pb Mg Pb Zn llowing table. An example is provided. Half-reactions Zn(s) → Zn²+ + 2e- Cu²+ + 2e → Cu(s) Cuzt +2e -> Cu(s) 2+ Pb²+ 2e-> Pb(s) Pb²+ + 2e--> Pb (s) 2 Ag+ 2e- Ag(s) Pb²2e Pb(s) Mg(s) Mg2+- 2e- Pb²+ + 2e => Pb (s) Zn(s)-> Zn²+ -2e- EⓇ +0.76 V +0.34 V +6.34V +0.13V Standard E cell -0.13V +2.37V -0.13V +0.76V +1.10 V +0.47V +0.13 V 40.80v +0.93 V +2.24V +0.63 V