Copper Synthesis

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The Loss and then Retrieval of Copper through Multiple Reactions Lab Partners: Justin Dunn and Alexis Almaguer Experiment #2 Section: 506 Intro: All science occurs within rules. One very important rule is that matter can neither be created nor destroyed and this rule will be expressed and proven in this lab by removing copper and then regaining it through multiple reactions, heating, and stirring. This experiment allows the students to learn the different types of reactions as well as learn new techniques within the laboratory such as vacuum filtration and handling hot glassware, but most importantly proves the law of conservation of mass. Materials and Methods: to begin the experiment a 50 ml beaker, hot plate, plastic funnel, aspirator,…show more content…
After a small amount of time the solution began to produce gas and the copper was being used up in the reaction. The solution turned an aqua like blue and eventually all of the copper had now been used into this blue solution which was copper nitrate and water, the gas being produced was nitrogen dioxide and the fume hood had removed it during the reaction. Next we slowly added drops of 6 molar sodium hydroxide to the solution until it became basic and turned a red piece of litmus paper blue. While we added NaOH the solution turned green indicating a new reaction had occurred and turned the litmus paper blue. We then began to heat and stir the solution until it changed color again and it turned black with a layer of water on top. This was the Cu(OH)2 decomposing into CuO and…show more content…
Using a Buchner funnel, a hose, and a suction flask we created a vacuum filtrator which we used to help remove the remaining liquid on the copper so that we may make a more precise measurement of the mass of the remaining copper. Our final mass of copper was .7951 grams. Results and Discussion: Initial Mass of Cu: .25 grams When we mixed the 5 ml of 6 molar HNO3 the copper had disappeared, indicating it had been used in the reaction. The copper had undergone a single replacement reaction and a decomposition reaction. Initial equation: Cu(s) + HNO3(aq) -> Cu(NO3)2(aq) + NO2(g) +H2O(l) Balanced: Cu(s) + 4HNO3(aq) -> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) The copper had replaced the Hydrogen in the HNO3 and the NO3 had also broken down into NO2 and O2- allowing the H+ to bond with it and create

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