Essay on Chemistry 1 Stoichiometry Lab

712 WordsNov 13, 20123 Pages
Stoichiometry 04/09/12 Chemistry I B Ms. Norton Introduction/Pre-laboratory Assignment: 1. Write out and balance each of the following equations. A. CuSO4 + Fe Cu + FeSO4 B. 3CuSO4 + 2Fe 3Cu + Fe(SO4)3 2. If Iron (III) Sulfate were formed, what mass of Copper would be expected and what is the limiting reagent? C. 2.26 g Cu D. Fe 3. If Iron (II) Sulfate were formed, what mass of Copper would be expected and what is the limiting reagent? E. 2.8 g Cu F. CuSO4 Driving Question: What compound is formed when you add 7 g of CuSO4 to 2 g of Fe? Goal: To correctly identify what compound is formed and how close it is to the theoretical yield. Materials: * Safety Goggles…show more content…
Let the copper settle to the bottom of the beaker and decant again. X. Dry the copper as your teacher directs and determine its mass. Record this mass. XI. Calculate the percent yield by using the theoretical yield that you determined in the pre-lab. Observations: Adding Iron to Copper (II) Sulfate * Got very hot * It started sizzling * Made greenish/turquoise bubbles * A brownish sludge formed These were all chemical reactions that took place. The reason that this is known is because of table 7.1 on page 219 in the textbook. Data: | Yield | Percent Yield | Theoretical: | 2.28 g Cu | 100 % | Actual: | 2.13 g Cu | 93.4 % | Data Analysis: When weighing the mass of our product you get 2.13 grams. Also when you figure out the percent yield you get 93.4%. Conclusion: I. The limiting reactant was 2.28 g Cu. Because iron is the limiting reactant. I know this because when the equation is done iron ends up being the limiting reactant. II. So iron would be the limiting reactant. You have unreacted iron that will mess up the weight. III. So the impurities were washed away and the experiment is contaminated. IV. It didn’t have anything to do with the reaction because it was a spectator ion. V. CuSO4 + Fe Cu + FeSO4 There are two main errors that could happen in this lab. The first being human error when weighing the elements. This would result in more reactants which would cause more products and a misreading
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