Compare The Formation Of Cu (Oh) 2 To The Rate Of Reaction Lab Report

907 Words4 Pages

This experiment was composed of five reactions: The formation of Cu(NO3)2, the formation of Cu(OH)2, the formation of CuO, the formation of CuSO4, and the formation of Cu(S). For Reaction 1 which was the formation of Cu(NO3)2, the mass of the copper wire was taken in an analytical balance so that it can be compared to the final mass of copper at the end of the experiment. The copper wire was bent slightly and was laid flat in a 250 mL beaker so that the 16 M HNO3 solution could cover the whole wire. In the fume hood, a disposable pipette was used to distribute about 4 mL of 16 M HNO3 into the beaker with the copper wire. The solution was stirred by rotating the beaker until the copper wire had completely dissolved and the toxic, brown NO2 gas …show more content…

The 250 mL beaker from Reaction 2 was heated on a hot plate, and stirred continuously for approximately 20 minutes until the reaction was complete, which is visible by the solution becoming clear the precipitate formed being all one dark brown/black color. The beaker was removed from the hot plate and the solid settled to the bottom. Once the solid had settled the solution was poured out into a waste beaker to leave just the solid in the beaker. To the solid, 200 mL of deionized water was added to a clean 400 mL beaker that was heated until just below boiling point. Once the water was sufficiently close to boiling, the beaker was taken off the hot plate and the water was poured into the 250 mL beaker with the solid. The solution was stirred and once the solid settled the liquid was poured into a waste beaker to leave just the solid in the beaker. When reaction 3 was completed the observations from the reaction were recorded in Table …show more content…

In beaker with the formed CuSO4 from Reaction 4, a piece of aluminum wire, which was bent into a circular shape, was placed in the beaker, and completely submerged in the solution. To this beaker a small stir bar was added along with 5 drops of 6 M HCl to start the reaction. This beaker was place onto the hot plate, covered with a watch glass, and the stir setting on the hot plate was turned on so that the stir bar moved the piece of aluminum wire around and hit it repeatedly. The wire began to have copper form on it and the stir bar hitting the wire would knock off the formed copper. Before the beginning of the next step the reaction had to be completed. If the reaction was happening at too slow of a rate or formation of copper was not happening the solution could be gently heated to help facilitate the reaction. After the reaction was done, the beaker was removed from the hot plate and the stirring rod was used to scrape off the copper that remained on the aluminum wire. The aluminum wire was removed from the solution and the liquid was poured carefully into the waste beaker, making sure not lose any of the copper. To dry out Copper, a steam bath was created using a 100 mL beaker filled with 50 mL of water and it was left to boil on the hot plate while copper was being washed with deionized water and ethanol. A wash bottle filled with deionized water was used to rinse the copper from the beaker into a small evaporating dish. No

More about Compare The Formation Of Cu (Oh) 2 To The Rate Of Reaction Lab Report

Open Document