2 1124 1159 302 D 01 M Cu 2 0001 M Cu 2 0065 00592 980 E 01 M Cu 2 001 M Cu 2

2 1124 1159 302 d 01 m cu 2 0001 m cu 2 0065 00592

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2+ -1.124 -1.159 3.02% D 0.1 M Cu 2+ 0.001 M Cu 2+ +0.065 +0.0592 9.80% E 0.1 M Cu 2+ 0.01 M Cu 2+ +0.020 +0.0296 32.43%
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difference in solution E which was 32.43%. the percent error of Solution E indicated that the values for my cell E were not precise and there could be some things that made this solution have a greater percent error. The E Cell values between Cells B and A changed with the dilutions of Cu 2+ . There was a decrease in E Cell from B to A. the experimental E Cell decreased by 0.025 V, while the calculated E Cell also decreased by 0.059 V. When cell B was diluted, there was less concentration, less ions, and therefore it makes the cell have a lower cell potential. The E Cell values between Cells C and A changed with the dilutions of Zn 2+ . There was a decrease in E Cell from C to A. the experimental E Cell increased by 0.044 V, while the calculated E Cell also increased by 0.059 V. When cell B was diluted there was an increase and therefore the cells potential increased. When the anode Zn 2+ was diluted it increased the cell potential because it lost electrons but when the cathode Cu 2+ was diluted, there was a gain in electrons which caused an increase in cell potential. There is a flow from anode to cathode in electrochemical cells and therefore the electrons moved from Zn 2+ to Cu 2+ . Some sources of error that could have caused our percent error to be increased is that maybe the electrodes were not cleaned correctly and therefore the readings could have been different than what the actual E cell is. Another source of error could be that there was not a precise dilution of the solutions. This could also affect the measured E cell values because it can either increase or decrease the E cell values.
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  • Spring '08
  • SMITH

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