The Magical Transformation of Aluminum to Copper... Just use Blue Water (Simplified)

Indroduction:


Chemical reactions are so much fun to experiment with. Especially watching the results that occur. The type of reaction that I would like to talk about is a single displacement reaction. This is where one element takes the place of another element in a compound. Ex AB+C --> AC+B. In our Experiment we used the equation Cu(SO4) (copper sulfate)+Al (aluminum --> Al(SO4) (aluminum sulfate)+Cu (Copper). So basically we mixed the Aluminum metal with a diluted Copper sulfate. And when we strained it. It ended up as a diluted Aluminum Sulfate and Copper metal. It was so cool. It was like BOOM... Copper out of Aluminum. Kind of like Jesus turned water into Wine but less epic.

3CuSO4 + 2Al --> Al2(SO4)3 + 3Cu

But this experiment is more than just fancy chemical reactions and all that jazz. We also did this for a learning experience, (though some people probably didn't actually learn that much most likely).

When the Aluminum is mixed with the diluted Copper Sulfate, the Aluminum takes the place of the Copper in the Copper Sulfate, making Aluminum Sulfate. This is because the Aluminum has a higher reactivity than the Copper, allowing the Aluminum to be like "Hey, I'm bigger than you. Get out of the way!!! (seductive voice) Hey Sulfate, hows it going. *wink wink*."

Purpose:

To determine the number of grams of copper that will be produced from an oxidation reduction reaction when you know the mass of Aluminum that reacted with a known amount of Copper(II) Sulfate Pentahydrate and to compare this to the actual yield of copper.

Materials:

• Safety gear (apron and goggles)


• 75-100 mL beaker


• 0.4-0.7 g Aluminum

• 7-10 g Copper(II) Sulfate Pentahydrate

• Bunsen burner


• stirring rod


• Erlenmeyer flask


• filter paper


• glass funnel

NOOOOOOOOO!!!!!
NOOOOOOOOOOO!!!!!!
NO NO!!!! GOD NO!!!!!
STOOOOOOOPPPPPPPPPPP!!!!!!!!!!

Before you do anything.... you need your safety materials.
Goggles and an Apron
Or else something bad might happen and you could DIE!!!!
Ok... maybe you won't die... but it can still be dangerous.
SO BEWARE!!!! and Be Safe!!!



Now... when you get your Safety Materials... You can Continue.

*Sigh of Relief*













Copper Sulfate

Procedure:

1. Obtain a medium sized beaker
2. Add 75-100 mL of water to beaker; set-up apparatus to heat your mixture over a Bunsen burner to begin heating.
3. Measure out about 15 g of Copper(II) Sulfate Pentahydrate (CuSO4 . 5H2O) and record the mass in the data table. Then slowly add the crystals to the heating water.
4. With a glass stirring-rod, stir the solution until the Copper(II) Sulfate Pentahydrate is dissolved.
5. While the copper sulfate crystals are dissolving one member of the group can go and get the foil. Carefully weigh out a piece of aluminum foil that weighs between 0.7 and 1.0 grams. Record the mass exactly into the data table (hundredths place).
6. Tear the foil into small pieces and carefully add it to the hot solution with continuous stirring until all the foil is placed into the beaker.
7. St irring frequently, allow the reaction to occur until you can't see any more sliver foil pieces. This will take 15 to 20 minutes, so be patient. Once you can't see anymore foil pieces, no matter how small, heat an additional 3 to 4 minutes. Then remove from heat.
8. Write your names around the outside edge of a filter paper (so you can claim it later), weigh and record the mass in the data table.
9. Use the filter paper and your funnel to filter the residue in the beaker, catching the filtrate into the Erlenmeyer flask provided.
10. Rinse out your beaker with a small (amount just covering the bottom of the beaker) of water to be sure you obtained all the product/residue
11. Remove the filter paper from the funnel and spread it out on a paper towel to dry ove rnight.
12. Clean and dry the glassware. Be sure the propane is turned off and Bunsen burner disconnected and put away. Straighten up your area.
13. Upon returning the next day, weigh the filter paper and dry the residue and record the mass in the data table, Throw the paper and residue away.
14. . Straining Process

Conclusion

When we finished our experiment, we weighed the amount of copper that we had, and it ended up weighing .41g. Here is a table showing masses of the stuff

Here is the Reaction that occurred again... just in case you are confuzzled and do not feel like scrolling back up to the reaction toward the top of the page

3CuSO4 + 2Al --> Al2(SO4)3 + 3Cu