exp 14 - increases so does the cell potential In part 2 of...

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Discussion: Experiment #14 In part 1 of this experiment, we tested the effects of temperature on cell potential. Our results had many variations and did not follow the expected pattern. For example we found the cell potential to be .488V at 22 degrees, but it increased to .503V at 3 degrees. The cell potential should have increased with the temperature. The balanced equation for this reaction is Pb(s) +Cu 2+ (aq) Cu(s) +Pb 2+ (aq). The graph gave a visual representation of how the cell potential changed with the temperature, which is a linear relationship. When we took out the outlier in our results which was the cell potential at 3 degrees, the graph was a straight line. From there we found the equation to be y=-25.13x-89223 and could calculate G, S, H, and K, which were quite different from the experimental values. The salt bridge used in the electrochemical cells allows the ions to flow between the cells, and gives a reading on the voltmeter. As temperature
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Unformatted text preview: increases, so does the cell potential. In part 2 of this experiment, we tested the effects of concentration on cell potential. Our measured and calculated results were very similar. We found the cell potential to be .488V with equal concentrations. It then increased to .527V with .1M of Pb and decreased to .455V with .1M Cu. This demonstrates that when the lower concentration is in the anode, the cell potential will increase and when it is in the cathode, it will decrease. Some possible sources of error in the experiment could have been the surfaces of the lead and copper electrodes. If there was any residue left from oxidation or the acid, it could affect the readings on the voltmeter. Another error could be in the salt bridge. If the electrons could not flow freely, it would also affect the cell potential reading....
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