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ANSWERS 1. Possible sources include the penny, the solution, the copper wires – by weighing before and after, students should be able to determine where the mass came from (i.e., if the loss of weight from the penny does not account for the whole gain on the dime, it must have gotten copper from the solution. Although the copper wires may also act as a source, they are not weighed separately, so this determination cannot be made empirically.) 2. 200 g CuSO4 / 1 L solution = 20% CuSO4 Or, molecular weight of CuSO4 = 159.607 g/mol [(Cu=63.546) + (S=32.065) + (O4=15.999 x 4) = 159.607] and 200 g CuSO4 / 159.607 g/mol = 1.25M CuSO4 3. Copper wire is used because copper is known for its properties as an excellent electrical conductor (it likely does not contribute significantly to the plating of copper on the dime). 4. The longer the experiment is run, the more copper plating will appear on the dime. 5. One would have to know what the content of each coin is – modern dimes actually contain copper, so you might still see it transferring to the penny. In order to make different metals move from different coins, one would need to optimize the electrolyte solution for that metal. This is why other metals are not plated in the commercial copper process – because of their different solubilities/chemistries, they either remain in solution or precipitate out. 6. One would need to start with a big anode (ie, not a penny!), adjust the electrolyte solution (more concentrated in both CuSO4 and acid than this experiment), and apply more power (this simple one-hour experiment can exhaust a 9V battery that delivers approximately 5.4 watts an hour). 7. Diagram of commercial-scale electrolytic refinement. Cu2+ Anode Cathode Cu2+ Cu2+ Anode Cathode Cu2+ Anode + Figure 10. Diagram of commercial-scale electrolytic refinement.PDF Image | Chemistry of Copper Electrolysis
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