Blue Tinge Experiment

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The data above should represent what was recorded and calculated from the experiment. Throughout the experiment, the solution began to have a blue tinge. At the end of the trials, the blue was obvious and this came from the reaction. This reaction is a result from the copper reacting to the sulfur acid. This creates a copper sulfate solution represented by the equation:
H2SO4 + Cu => CuSO3 +H2O
When the copper sulfate is hydrated, it turns blue. The copper sulfate is in water after the reaction, so the water hydrated the copper sulfate. This was also seen in a previous experiment when heating copper sulfate hydrate and then rehydrating it. The change in mass in trials one, two, and three are .072 g, .030 g, and .021 g respectively. The change …show more content…

Finding the number of copper atoms means dividing the amount of electrons lost by two. This gets 1.60x1020 atoms, 2.76x1020 atoms, and 3.57x1020 atoms. To find copper atoms pre mole of copper lost, divide the copper atoms lost by the change in moles of copper. This gives 1.28x1023 atoms, 5.87x1023 atoms, and 5.39x1023 atoms. The average number of atoms is 4.18x1023 atoms. The listed numbers should be close to Avogadro’s number. This is not the case because there are discrepancies during testing. The percent error for the trials are 76.5 %, 2.50 %, and 10.5 % respectively. The percent error for the average is 29.9 %. The percent errors for trials two and three are reasonable because of how close they are to Avogadro’s number. The percent error for trial one was an outlier. During the first trial, I had trouble making the LabQuest working correctly since it kept running at 18 seconds instead of the 180 seconds. The repeated dipping of electrodes and constant restarting of the first trial may have skewed results. The trials afterwards ran with relative ease compared to the first trial. Because the other trials ran better than the first, the numbers calculated in the end for those trials were closer to Avogadro’s number. The experiment shows by knowing the current and the masses of copper before and after electrolysis, one can determine Avogadro’s number under the right

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