The Faraday constant F is a fundamental constant in electrochemistry that represents the charge of one mole of electrons. It is named after the famous scientist Michael Faraday. The Faraday constant is used to relate the amount of electric charge transferred during an electrochemical reaction to the amount of substance in moles that is reduced or oxidized.The Faraday constant is approximately 96,485 Coulombs per mole of electrons C/mol e- . This value is derived from the charge of a single electron approximately 1.602 x 10^-19 C multiplied by Avogadro's number approximately 6.022 x 10^23 mol^-1 .To calculate the Faraday constant using copper electroplating as a case study, you would need to perform an experiment where you measure the amount of electric charge passed through a copper sulfate solution and the mass of copper deposited on the cathode.Here's a step-by-step process:1. Set up an electroplating cell with a copper anode and a cathode the object to be plated immersed in a copper sulfate solution.2. Connect the anode and cathode to a power source such as a battery or power supply to create an electric current.3. Allow the electroplating process to proceed for a specific amount of time, during which the copper ions in the solution are reduced to copper metal at the cathode.4. Measure the electric current in amperes and the time in seconds for which the electroplating process was carried out. Multiply the current by the time to obtain the total electric charge in Coulombs passed through the solution.5. Carefully remove the cathode from the solution, clean it, and measure the mass of the deposited copper in grams .6. Convert the mass of deposited copper to moles using the molar mass of copper approximately 63.55 g/mol .7. Finally, divide the total electric charge in Coulombs by the number of moles of deposited copper to calculate the Faraday constant in C/mol e- .This experimental value should be close to the accepted value of 96,485 C/mol e-. Keep in mind that experimental errors and impurities in the copper sulfate solution can affect the accuracy of the calculated Faraday constant.