Retrieving Copper
7/19/13
Charlie, Georgie, Ben
Dr. Forman
Lab Questions:
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| Group Data Table |
1. a. The observational evidence that leads us to think that the reaction was incomplete because when you heat copper, atoms of copper don't leave, they just change.
b. I could revise the procedure so that more copper (II) oxide could form by heating copper for a longer amount of time, so more copper can combine with oxygen.
2. a. The mass of the original powdered copper sample that reacted when we heated it was 96%.
b. The percent of the total copper sample that reacted was 85%.
3. a. Cu2+ + Zn --> Cu + Zn2+
b. i. The reactant that was oxidized was Zn.
ii. The reactant that was reduced was Cu2+.
iii. The reducing agent is Zn.
iv. The oxidizing agent is Cu2+.
4. a. When we added zinc to the solution there was a reaction and caused a dark red color, and was brittle, like a copper color.
b. What caused the changes we observed in the solution was the theory that a more reactive metal will cause a reaction in a less reactive solution. And in this cases zinc is more reactive than copper.
c. Once the solution changed to a clear color, it proved that Cu2+ ions int he solution reduced to Cu. And the Zn had oxidized to become Zn2+.
5. a. The resources that were used up in this recovery process was Cu2+ ions and solid Zn.
b. Cu2+ reduced to Cu, and Zn oxidized to Zn2+ in the solution.
Aggregated Class Data:
Before our experiment to retrieve copper, the class as a whole believed that when we heated copper that we converted all the copper, but really only about 30% of the copper converted. And 50%-70% of the copper didn't converted. In the unconverted copper, most groups got about 0.70g of unconverted copper and other groups got more around 0.60g. However, when we converted copper, most groups got about 0.24g, and many more got a higher number around 0.34g. After we retrieved copper we realized that atoms are never destroyed or made, but just changed.
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| Class Aggregated Data |
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