I completed an electroplating lab for my chemistry class. In the lab, I set up an electrolytic cell to plate copper metal (from a copper strip) onto 2 other metal objects: one was a quarter; the other was an ungalvanized iron nail. The electrolyte solution I used was Copper Sulfate (1.0 M). Knowing this, can someone help me with this question?
1. Electrolytic cells like we set up in this lab have both oxidation and reduction reactions happening in the same apparatus. In an electroplating apparatus, the same metal is both oxidized and reduced. For our experiment, write the oxidation and reduction half reactions that are occurring. In writing your reactions, make sure they are balanced and include the physical states of the ions and elements.
In this process,reduction occurs at the cathode whereas oxidation occurs at the anode Oxidation happens at the anode... View the full answer