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The primary objective of this experiment was to explore the recyclability of copper through a series of chemical reactions. Despite theoretical expectations that the amount of copper should remain constant throughout the reactions, practical factors such as filtration, decanting, and incomplete reactions may alter the final yield. The experiment involved oxidation-reduction reactions, specifically decomposition and displacement, crucial processes in the extraction and recycling of elements.
Materials and Methods:
The beaker was swirled occasionally until no fumes were produced.
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A 2g sheet of zinc metal was added, initiating a displacement reaction. The reaction mixture was placed under the hood until the zinc metal completely reacted.
Calculations and Formulas:
Results:
Discussion: The experiment involved oxidation-reduction reactions, starting with the dissolution of copper in nitric acid.
This reaction can be represented as follows: Cu(s)+4HNO₃(aq)→Cu(NO₃)₂(aq)+2NO₂(g)+2H₂O(l)Cu(s)+4HNO₃(aq)→Cu(NO₃)₂(aq)+2NO₂(g)+2H₂O(l) Here, copper is oxidized from 0 to +2+2 oxidation state, and nitrogen is reduced from +5+5 to +4+4 and +2+2.
The subsequent addition of sodium hydroxide results in the formation of copper hydroxide, which is further dissolved in sulfuric acid to produce copper sulfate: Cu(OH)₂(s)+2H₂SO₄(aq)→CuSO₄(aq)+4H₂O(l)Cu(OH)₂(s)+2H₂SO₄(aq)→CuSO₄(aq)+4H₂O(l) The zinc metal, when added, displaces copper from copper sulfate in a redox reaction: Zn(s)+CuSO₄(aq)→ZnSO₄(aq)+Cu(s)Zn(s)+CuSO₄(aq)→ZnSO₄(aq)+Cu(s)
The percentage yield was found to be 94%, indicating the efficiency of the experimental procedure. This high yield suggests that the reactions proceeded with minimal side reactions or losses during filtration and decanting.
The experiment demonstrated the recyclability of copper through a series of oxidation-reduction reactions. The high percentage yield indicates the success of the experimental procedure. The understanding of these chemical processes is crucial for the efficient extraction and recycling of elements, contributing to both scientific and industrial advancements.
Upon reaction with nitric acid, solid copper underwent a chemical transformation, resulting in a blue solution of aqueous cupric nitrate, water, and the emission of nitrogen oxide, a brown and toxic gas. This reaction combines elements of a single displacement reaction and a decomposition reaction, and it can be represented as follows:
Upon reaction with nitric acid, solid copper underwent a chemical transformation, resulting in a blue solution of aqueous cupric nitrate, water, and the emission of nitrogen oxide, a brown and toxic gas. This reaction combines elements of a single displacement reaction and a decomposition reaction, and it can be represented as follows: Cu (s) + 4HNO3(aq)→Cu(NO3)2(aq)+2NO2(g)+2H2O(l)Cu (s) + 4HNO3(aq)→Cu(NO3)2(aq)+2NO2(g)+2H2O(l)
The cupric nitrate solution then underwent a double displacement reaction with aqueous sodium hydroxide, producing blue cupric hydroxide and aqueous sodium nitrate: Cu(NO3)2(aq)+2NaOH(aq)→Cu(OH)2(s)+2NaNO3(aq)Cu(NO3)2(aq)+2NaOH(aq)→Cu(OH)2(s)+2NaNO3(aq)
The resulting mixture of copper hydroxide and sodium nitrate was heated, leading to the formation of copper oxide (a black precipitate) and water through a decomposition reaction: Cu(OH)2(s)→CuO(s)+H2O(l)Cu(OH)2(s)→CuO(s)+H2O(l)
The filtrate containing copper oxide (CuO) was then subjected to a double displacement reaction with sulfuric acid, resulting in a blue mixture of copper sulfate and water: CuO(s)+H2SO4(aq)→CuSO4(aq)+H2O(l)CuO(s)+H2SO4(aq)→CuSO4(aq)+H2O(l)
Subsequently, a 2g zinc metal was introduced into the copper sulfate and water mixture, undergoing a single displacement reaction that produced copper and zinc sulfate: CuSO4(aq)+Zn(s)→Cu(s)+ZnSO4(aq)CuSO4(aq)+Zn(s)→Cu(s)+ZnSO4(aq)
After the copper was cooled to room temperature, washed with methanol, decanted, washed with acetone, decanted again, and dried using a water bath, the pre-weighed 70.00g beaker containing the recovered copper was weighed. The mass of the copper and beaker together was determined to be 70.47g. The mass of the recovered copper was calculated by subtracting the mass of the beaker from the combined mass of the beaker and the recovered copper.
The percent yield was then calculated as the ratio of the actual yield (mass of the recovered copper) to the theoretical yield (initial mass of the copper wire), multiplied by 100.
Laboratory Report on Copper Recycling: Experimental Procedures and Analysis. (2024, Feb 28). Retrieved from https://studymoose.com/document/laboratory-report-on-copper-recycling-experimental-procedures-and-analysis
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