8.docx - CH 204 – Introduction to Chemical Practice Experiment 8 – The Copper Cycle Lucas Stephen Elbaum Melissa November 7 2019 INTRODUCTION The

8.docx - CH 204 – Introduction to Chemical Practice...

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CH 204 – Introduction to Chemical Practice Experiment 8 – The Copper Cycle Lucas Stephen Elbaum Melissa November 7, 2019 INTRODUCTION The purpose of this experiment was to react copper to form 4 different copper compounds before returning back to its original form. Observe and record physical and chemical changes of the reactions. The percent recovery of the final copper was determined and that there were balanced chemical equations for the reactions. The objectives were acid-base, redox, and precipitation reactions for successive copper-based compounds. Calculation of the percent recovery of the copper product. % balanced chemical equations from classification of each reaction in cycle. A historical perspective is that since 1954, 56 countries have done an analysis on the copper cycle who have pretty much all of the copper stock in the whole world. 1 What we use the copper cycle for is to monitor the rates at which the copper can be manufactured, fabricated or extracted from the earth. 2 RESULTS & DISCUSSION To begin the reaction, copper metal was dissolved in nitric acid which was actually the nitrate ions oxidizing the copper ions to form NO 2 gas in the process which was the gas that made the brown smoke, while at the same time it formed a water soluble salt in a blue solution which was the Cu(NO 3 ) 2 . In the next step, Cu(NO 3 ) 2 was reacted with NaOH which produced the light blue salt of Cu(OH) 2 and also a colorless salt of NaNO 3 which was dissolved inside of the solution. After heat was applied to the Cu(OH) 2 , it caused a black solid to form which was
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insoluble in the solution from the CuO. After that, when H 2 SO 4
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