please answer #4

Electrodes Half-reactions Zn Cu Zn(s) -- Zn. 2 Cue Cuis -1.10V Cu +0.76 V +0 34 V 70.340 Pb Ag 8 38 22 23 1 +0.13 tou (s)-> Cu2+ +2e P6 +2e Cu(s) Pb (s) > Pb2+ + 2e- Agt Mot+222 Mau Pb(s) Pb2+ + 20 2n+2 +2e Zuls) Pb Mg PolsterP679 26 -0.131 +0.47 +0.80 +1.73 +2.37v / 2,24v 1-0.764/-0.631 HO.131 Pb Zn 40.13 | DDAAN DATA TABLE Results of Parts I and I Cu/Pb X/Pb YIPb Average cell potential (V) 10.0177 1.0757 0.4397 Results of Part III Cu concentration Pb/Pbly Average cell potential (V) 10.01 0.0437 DATA ANALYSIS value. 1. (Part 1) Compare the average cell potential, for your Cu Pb cell with the E'est that you calculated in the pre-lab exercise. Explain why your cell potential is different from the text 2. (Part II) The unknown metals X and Y were either magnesium, silver, or zine. 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/Pbl2 cell to complete the following calculations. a. Use the cell potential for the Pb-Pbl cell and the known [Pb?") to calculate the [Pb2') in equilibrium with Pblz. b. Use the original diluted [Pb') and [l] to calculate the [1] in solution c. Use your data to calculate the key of Pbl d. The accepted value of the K of Pblz is 9.8 x 10". How does your experimental Kop of Pbly compare with the accepted value