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Electrochemistry Essay

587 words - 3 pages

Electrochemistry: Voltaic Cells
Erica Lieser
Kendall Mello
CHM145D
Lauren Bottorf
April 25, 2013
Part 1
Table 1:
Cathode | Anode | Observed Potential (V) | Standard Cell Potential (V) | (%) Relative Error |
Copper | Zinc | 0.91 | 1.10 | 17.3 |
Copper | Magnesium | 1.33 | 2.71 | 50.9 |
Zinc | Magnesium | 0.48 | 1.61 | 70.2 |
Copper | Aluminum | 0.65 | 2.00 | 67.5 |
Aluminum | Magnesium | 0.74 | 0.71 | 4.23 |

Table 1 shows the measured potential readings and the standard cell potentials for all of the combinations above. The predicted Cu/Al potential was 1.09V which was much higher than the measured value of 0.65V. The prediction was made based on the Cu/Mg potential of 1.33V and the Al/Mg potential value of 0.74V. The ...view middle of the document...

01 M, it means that a large amount of the solution was water. This causes the observed voltages to be smaller than what they should be.
From part one, the reduction reactions and half-cell potentials are as follows:
Reduction Reaction | Half-Cell Potentials |
Cu2+(aq) + 2e- → Cu(s) | 0.34 |
Zn2+(aq) + 2e- → Zn(s) | -0.76 |
Mg2+(aq) + 2e- → Mg(s) | -2.37 |
Al3+(aq) + 2e- → Al(s) | -1.66 |

Part 2
Table 2:
Cathode Concentration (M) | Anode Concentration (M) | Observed Potentials (V) | Nernst Voltage | Percent Error |
1.0 Cu | 0.001 Zn | 0.82 | 1.19 | 31.10% |
1.0 Cu | 1.0 Zn | 0.87 | 1.10 | 23.00% |
0.001 Cu | 0.001 Zn | 0.83 | 1.10 | 24.50% |
0.001 Cu | 1.0 Zn | 0.82 | 1.01 | 18.80% |

Table 2 shows the potential values for two different concentration combinations of zinc and copper. The potentials mainly stayed around 0.83V, however the highest potential came from the combination of 1.0 M of both Zn and Cu which was 0.87V. These changes DO/DO NOT AGREE WITH MY EXPECTATIONS, WHY??
Balanced reaction: Zn(s) + Cu2+(aq) → Cu(s) + Zn2+(aq)
4.
Part 3
Table 3: 0.001 M Zn (Anode)/1.0 M Cu (Cathode)
Number of EDTA Drops | Observed Potentials (V) |
0 | 0.86 |
5 | 0.91 |
10 | 0.87 |
15 | 0.87 |
20 | 0.85 |

After the addition of EDTA, there was not a common trend in the data. At first the potential increased but then slowly decreased as more drops were added. EXPECT?
Table 4: 1.0 M Zn (Anode)/0.001 M Cu (Cathode)
Number of EDTA Drops | Observed Potentials (V) |
0 | 0.76 |
5 | 0.77 |
10 | 0.77 |
15 | 0.77 |
20 | 0.77 |
After the addition of EDTA, there was not a common trend in the data. At first the potential increased but then slowly decreased as more drops were added. EXPECT?
EDTA was used in this lab because it is an effective complexing agent for metal ions. USE TEXT.

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