Copper Lab Report

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Tarrant County College, Fort Worth *

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1441

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Chemistry

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Jan 9, 2024

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docx

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Kat Castro Luis Veliz 11/03/2022 Cycle of Copper Objectives: Learning how to utilise both percent recovery and different types of reactions through copper. Procedures: Followed as directed in the notebook. Results: Table 1 : Initial and Final Amounts of Copper. Copper Granules Started With 0.4 g Copper Granules Ended With 0.04 g The table above shows both the initial amount of Cu granules, 0.4g, and the final amount of Cu granules, 0.04g. Table 2 : Procedure Analysis Questions. Question Answer What products are present in the solution once the reaction is complete? (Regarding reaction one). Cu(NO3)2+2NO2+2H2 O

Reference the balanced chemical equation for Reaction (2) above. In addition to Cu(OH)2, what other chemical product formed in the solution? NaNO3 Consider both Reaction (2) and Reaction (3). Which products are removed during the washing and decantation steps (step #11 - #12)? NaNO3 Which products were formed upon the addition of H2SO4 in step #13? CuSO4, H2O What type of reaction is Reaction (5)? single displacement Which element is being oxidized and which element is being reduced in Reaction (5)? Zinc is being oxidized and Copper is being reduced. What color is the recovered metallic Cu? Does it resemble your starting material from step #1? It was a darker colour (redder) than what we started off with. Not as "orange-y" The table above shows both the questions and answers to the procedure analysis questions. Analysis: As shown above in Table 1, the precent recovery of the copper was only 10%. It is technically possible to get a calculation of over 100% recovery, but that just means that there was extra zinc still in the reaction. There were also plenty of observations made during different

reactions. Starting off with Cu(s)+HNO3, an oxidation-reduction reaction, there was a change in colour, going from orangish to blue. Along with yellow-orange fumes and being released. Next is Cu(NO3)2+NaOH, a double replacement reaction. The physical changes were the colour change, it went to a very dark blue, maybe black. It also had chunks near the bottom and got extremely thick. Next was Cu(OH)2+heat, a decomposition reaction. The physical attributes of the reaction was that it was still extremely dark and had small particles of the bottom. Next was CuO+H2SO4, a double displacement reaction. The physical attributes were that it changed to a very light blue. The last reaction was CuSO4+Zn, a single displacement reaction. The particles at the bottom turned reddish and while the reaction unfortunately never made it completely clear, but it was mostly transparent. Calculations: Determining the Amount of Copper Recovered in Grams. Erlenmeyer Flask with Recovered Metallic Copper - Empty Erlenmeyer Flask = Recovery of Metallic Copper 76.01 g-75.97g= 0.04 g Determining the Percent of Copper Recovered. Mass of Cu Recovered/ Original Mass of Cu Granules x100% = Percent Recovery 0.04/0.4 = 10% Discussion and Conclusions: While in theory it is impossible to have over 100% recovery, it is possible to not oxidise all the zinc and that also would count towards the calculations. There were plenty of different reactions, from an oxidation-reduction reaction (reaction 1) to a double

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replacement reaction (reactions 2 and 4) to a decomposition reaction (reaction 3) and a singular displacement reaction (reaction 5). While there were quite a bit of changes happening during the reactions, it can be seen in the last reaction that the copper was being reduced and the zinc was being oxidised. In the recovery, the copper is gaining electrons while the zinc is losing some, which leads to why the oxidation-reduction relationship between the two is so.