lab 3.docx

lab 3.docx - Lab Report#3 Calculations 1 Determine the mass...

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Lab Report #3 Calculations 1. Determine the mass of Cu metal produced: (Experiment 1) Mass of Cu = 102.365g - 101.273g = 1.092g (Experiment 2) Mass of Cu = 55.447g – 55.180g = 0.267g 2. Mass of Zn reacted: (Experiment 1) Mass of Zn reacted = 4.269g – 3.222g = 1.038g (Experiment 2) Mass of Zn reacted = 4.092g - 2.952g = 1.140g 3. Determine percent of Cu in copper chloride: (Experiment 1) Percent Cu = (1.092g/2.01g) x 100% = 54.32% (Experiment 2) Percent Cu = (0.267g/2.01g) x 100% = 13.27% 4. Determine the mass of Cl in the copper chloride: (Experiment 1) Mass of Cl = 2.01g - 1.092g = 1.016g (Experiment 2) Mass of Cl = 2.01g – 0.267g = 1.743g 5. Determine percent of Cl in copper chloride: (Experiment 1) Percent Cl = (1.016g/2.01g) x 100% = 50.47% (Experiment 2) Percent Cl = (1.743g/2.01g) x 100% = 58.42% 6. Calculate the formula and mass percent of Cu and Cl for each compound below. Compare experimental percentages with those of the table. Determine the best fitting empirical formula. Compound Formula Mass % Cu % Cl CuCl 99.00 g/mol 64.19% 35.81% Cu 2 Cl 162.55 g/mol 78.19% 21.81% CuCl 2 134.45 g/mol 47.26% 52.74% Cu 2 Cl 3 233.45 g/mol 54.44% 45.56% Cu 3 Cl 2 261.54 g/mol 72.89% 27.11%

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(Experiment 1) Percent Cu = 54.32%; Percent Cl = 50.47%. Empirical formula Cu 2 Cl 3 (Experiment 2) Percent Cu = 13.27%; Percent Cl = 58.42%. Empirical formula CuCl 2 (CuCl 2 is closest, but really none of them fit) Questions: 1. Which of the reactants in your experiment was the limiting reagent? Which of the reactants was present in excess?
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• Spring '12
• McFadden

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