# E ¬∞ Of Three Voltaic Cells Essay

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In this experiment, the E° of three voltaic cells, and two concentration cells was calculated using a voltage probe. These E° readings were used to determine the identities of two metals, X and Y, which were used as anodes in two of the voltaic cells. The Nernst equation was then used to determine the Ecell of a copper concentration cell, and the concentration of Pb2+ in a lead concentration cell. Using the concentration of Pb2+ from the lead concentration cell, the Ksp of PbI2 was determined. The theoretical E° of the Cu-Pb voltaic cell was calculated by using the equation E°cell = E°cathode - E°anode. The cathode in part A was copper, while the anode was lead. The E° of copper, was 0.34V, and the E° of lead was -0.13V, and subtracting the E° of lead from the E° of copper resulted in the theoretical E°cell value of 0.47V. The average corrected E°cell for the Cu-Pb voltaic cell was found to be 0.492V, which is quite close to the theoretical value of 0.47V. The average corrected E°were recorded in the following table: Run Cu-Pb Pb-”X” Pb-”Y” Cu Conc. Pb Conc. 1 0.488 0.985 0.396 0.034 0.198 2 0.481 1.022 0.394 0.028 0.138 3 0.507 1.042 0.390 0.036 0.110 Average 0.492 1.0163 0.3933 0.03267 0.149 The two half-reactions for the CuPb voltaic cell were found to be: Cu2+(aq) + 2e- → Cu(s) Pb(s) → Pb2+(aq) + 2e- Net Ionic Equation: Cu2+(aq) + Pb(s) → Cu(s) + Pb2+(aq) The Cu-Pb voltaic cell can be denoted in standard cell notation as: Pb|Pb2+||Cu2+|Cu The theoretical E° of the