Collin County Community College District
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This 4 page Class Notes was uploaded by Mariah Olgin on Wednesday September 21, 2016. The Class Notes belongs to Math 2414 at Collin County Community College District taught by Sarah Lynch in Fall 2016. Since its upload, it has received 7 views.
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Date Created: 09/21/16
1 Lab Report: Recycling Aluminum Chemically Lab Report: Recycling Aluminum Chemically Mariah Olgin CHEM 1411 2 Lab Report: Recycling Aluminum Chemically Background Information: Aluminum is one of the most abundant elements on earth. Even though it is quite abundant it takes a significant amount of energy and resource to process refine and use aluminum in everyday and functioning applications. Many companies instead have ways of chemically recycling the aluminum so that it can be used again. This process takes much less time and energy than it would if it were to be mined and refined for its ore state. In this lab we will be using a chemically process involving acid to break down the original aluminum into Alum crystals. The ultimate goal is to produce the highest yield of alum crystals based on the original amount of aluminum. 100% is the perfect amount, that would be the theoretical yield of alum. In real life applications for business, the higher percent yield will have the least amount of resources used in recycling the aluminum and the most potential for money to be made by the product. Procedure: 1.0002 g of the aluminum foil was measured out and placing it in the 250 mL beaker. Next, 25mL of KOH was added to the same beaker and the reaction that took place was observed under the fume hood. After 5 minutes, the beaker with the solution was placed on a hot plate and gently heated. There were a few times when the liquid level was lowering that small amounts of deionized water was added. The color of the reaction was observed. Next, the beaker was lifted and the solution poured into the vacuum filter in the Buchner Funnel to filter out any undissolved pieces. The reaction beaker was rinsed and poured the rinse back through the filter. The 3 Lab Report: Recycling Aluminum Chemically filtrate was then placed into a clean beaker and the flask was rinsed with 10mL of deionized water. This was added into the same beaker. The solution was let to cool. Next, 20mL of Sulfuric Acid was stirred in. The reaction was heated until it was clear. With a prepared ice water bath, the beaker containing the filtrate was placed in the bath for 15 minutes. During this time, the filter paper was weighed. Then with the same vacuum filtration system, the mixture was again filtered. The solution was rinsed with an ethanol-water solution with 12mL ethanol and 12mL of deionized water. The vacuum was applied to dry the remaining crystals until completely dried. These alum crystals produced were then weighed. Finally, we showed our finishing product to our lab instructor before calculating our percent yield. Results: Initial Mass of Al: 1.0002 grams Al + KOH Observations (color?): boils, steams as Al dissolves, turns black when fully dissolved Reaction complete when heated: turns clear On Filter Paper: small black powder substance Color of Filtrate: clear + H 2O :4solid white substance formed then mixed in till solution was milky white, turned clear again when heated. Alum Crystals: 8.599 grams Theoretical Yield: 17.57 grams Percent Yield (Actual/Theoretical x 100): 48.9% 4 Lab Report: Recycling Aluminum Chemically Conclusion: In this lab we were successfully able to simulate a process similar to how Aluminum is recycled professionally for businesses. The theoretical production we initially predicted for alum crystal mass was 17.57 grams given the initial mass of the aluminum by dividing the initial by the molar mass of Aluminum and them multiplying that by the molar mass of Alum. We received a real life production of only 8.599 grams giving us an 48.9% percent overall yield to alum production. Toward the end of the lab when the final amount of alum crystals was measured and the crystals were transferred from the filter and paper to the balance so the mass could be weighed, if any fell or was knocked off then that would have lowered our results. Also, had the alum crystals been given more time to grow then our percent yield could have been higher. When we heated out initially solution we brought out liquid to boiling instead of a gentler heating. There was also the potential for slight variations in measurements. Overall our yield compared to our theoretical was not very high. In a real life business, they would only be producing half of the Alum that they could be potentially be making, but of in business the making the most possible leads to a higher profit overall.
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