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Synthesis of Copper Compounds and Isolation of Copper from Metallic Copper

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Synthesis of Copper Compounds and Isolation of Copper from Metallic Copper Thien Nguyen ID: 20299974 TA: Chris Gordy Partner: Daniella Guirgis Section - 007 Introduction The chemical industries are always looking for ways to increase how much material they receive in relation to how much they put in. It is extremely important for chemical industries that they get the most they want out of what they put in, in terms of chemical reactants, value of by products, usage of equipment to retrieve the materials, the percent of yield (Department of Chemistry, 2009). In this experiment, the chemical process that isolates copper will be examined. These chemical processes are: the synthesis of copper (II) nitrate, copper (II) hydroxide, and the conversion copper (II) oxide, the formation of copper (II) sulphate, the formation of copper metal in a solution, and the removal of Zinc (Department of Chemistry, 2009). Cu-->Cu(NO3)2-->Cu(OH)2-->CuO-->CuSO4 5H2O-->Cu To determine whether or not the method/processes are efficient, the percent yield/recovery is then calculated from the recovered copper and the mass of initial copper. (Department of Chemistry, 2009). Experimental Procedure The experimental procedure used for this experiment was outlined in the CHEM 120L lab manual, Experiment #1. All steps were followed without deviation. ...read more.


oxide. In this reaction the acid, H2SO4 reacts with the basic copper (II) oxide in a neutralization reaction to create CuSO4, copper (II) sulphate salt, and water. The balanced chemical equation for this reaction is: CuO(s) + H2SO4 (aq) -->CuSO4 (aq) + H2O(l) `The fifth reaction that takes place forms Cu metal from CuSO4. To do this, zinc was added to the aqueous solution of CuSO4. During this reaction, it finally recovers some of the copper that was started with in the form of a brown precipitate. The solution also turns clear eventually from blue as the copper is being precipitated and being replaced with zinc, forming zinc sulphate. Zn(s) + CuSO4(aq) --> Cu(s) + ZnSO4 (aq) The above reaction is another redox reaction. This is because zinc, started off with an oxidation state of 0 before the reaction, and after the reaction zinc ended up with an oxidation state of +4, thus zinc loses 4e- and is in turn oxidized. In the case of copper, it has an oxidation state of 10 in CuSO4 and after the reaction it ended up with an oxidation state of 0, therefore copper is reduced as it gains 10e-. ...read more.


hydroxide. Also, NaOH is very basic, and very corrosive, therefore it does pose a risk. Minimizing spillage is important for chemical safety. 3. Suggest a reason for allowing the last traces of water to evaporate slowly rather than rapidly expelling the water by intense heating. One reason for allowing the last traces of water to evaporate rather than rapidly expelling the water by intense heating so that the energy from boiling the water does not expel some of the copper precipitate out of the dish. Conclusion In conclusion, the methods are being experimented with to synthesize and isolate are effective when using them for large quantities of substances. Mass production of these compounds would be best for employing these methods, as many of the processes synthesis do take time and thus, using as much material to synthesize or isolate, as possible would minimize down time. For small quantities, other methods should be used. In terms of how useful these methods are for the chemical industry, these methods are relatively simple and will be able to do the job for mass production of synthesized compounds or even isolating an element. Although the results from this experiment were erroneous, there is no doubt that the simplicity of the processes is invaluable to the chemical industries. ...read more.

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