100 Of The Copper Metal example essay topic

Intro In Lab #5 five we will be exploring the cycle of copper through many chemical reactions. What we are going to do is take a piece of copper metal put it through a series of reactions that change it's state of matter and chemical formula, but in the end, we will return it to it's normal solid state. The idea of this lab is to try to recover as close to 100% of the copper we started with. Theoretically, this is possible, but for inexperienced college students, retrieving 100% of the copper metal is near impossible. Cu (OH) 2 (s) "^3 CuO (s) + H 2 O (aq) 4. CuO (s) + H 2 SO 4 (aq) "^3 CuSO 4 (aq) +H 2 O (aq) 5.

CuSO 4 (aq) + Zn (s) "^3 Zn SO 4 + Cu (s) At the end of reaction number five we should have close to 100% of the copper we started out with. Meth Obtain as close to. 5 g of copper wire, and record the mass to the closest mg. Make sure the wire is bent so it will lay as flat as possible in the bottom of a 250 mL beaker. Then go to!

SSthe hood!" and add 4 mL of 16 M HNO 3. Swirl the HNO 3 around in the beaker with the copper until it has completely dissolved and you are left with a green / blue liquid. Then add 30 mL of 3 M NaOH and heat the solution on a ring stand with a Bunsen burner. The blue / green jelly will turn in to sort of a black dirt at the bottom of the beaker, make sure to stop boiling when the jelly turns black.

Decant all excess liquid in the beaker. Do not remove any black precipitate. Add approximately 200 mL of hot deionized water to the black precipitate. Decant all excess liquid again. Add 15 mL of 6 M H 2 SO 4 and then under! SSthe hood!" add 2 g of Zinc metal to the solution.

Once the Hydrogen has stopped bubbling add 10 mL of HCl. Decant all excess liquid and transfer Copper metal to a glass dish and wash with deionized water. Rewash Copper metal with 5 mL of Methanol. Decant and dry Copper metal on a hot plate, weigh and record results to nearest mg. ResuOriginal Mass of Cu = . 486 mass of Cycled Cu = .

480 g 1. In the first reaction the was brown smoke and the copper turned into a light blue / green liquid. 2. In the second reaction the solution turned into a clear blue liquid. 3.

In the third reaction when the solution was heated a blue jelly formed and then a black precipitate formed at the bottom of the beaker. 4. In the fourth reaction the black precipitate turned into a light blue liquid once again. 5. In the final reaction the clear blue liquid turned into a copper colored metal, known as copper. Calc% Recovery = Mass Recovered / Initial Mass 10098.76% = .

480 g/. 486 g 100 Disc For inexperienced college students our lab group did a great job in recovering as much of the copper as possible, our group recovered 98.7%. This number may be too high and we may not have actually recovered as much copper as we think, one accident could have been made when drying the copper, and not letting enough of the water evaporate, this could lead to a falsely high percent recovery. But if we did let all the water dry and we did get our results some reasons for not getting the total 100% recovered we may have decanted some of the black precipitate when decanting, we may have also burned up some of the copper in the drying process and last the transfer of copper from the beaker to the glass plate may have not gone as smoothly as we planned and we may have not gotten all of the copper..