Electroplating is a valuable industrial process that allows metals to be plated onto other materials using an electrical current. In this activity, an electrolytic cell is used to electrolyze a solution of copper(II) sulfate. A voltage source is connected to two copper strips, and the strips are placed into the solution of copper ions. The energy from the voltage source will cause a redox reaction to occur within the cell. At one electrode, copper(II) ions will be reduced to elemental copper, and at the other electrode, elemental copper will be oxidized to form copper(II) ions. By measuring the initial and final masses of the two electrodes, the amount of copper oxidized (and reduced) during the experiment can be calculated. This data, together with information about the amount of current that passed through the cell, will be used to calculate values for Avogadro's number and the Faraday constant. Includes materials for 15 setups.
Chemical Contents:
Copper Sulfate Pentahydrate
Copper Metal Strips
Sulfuric Acid Solution
Additional Materials Required:
Ammeter
Analytical Balance
150 mL Beaker
Battery
Timer
100 mL Graduated Cylinder
Isopropyl Alcohol
Wires and Alligator Clips
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