To determine the Faraday constant F using the electroplating of copper on a platinum electrode, we need to follow these steps:1. Calculate the total charge Q passed through the cell.2. Determine the moles of copper deposited n .3. Use the moles of copper and the total charge to calculate the Faraday constant.Step 1: Calculate the total charge Q passed through the cell.Q = current I time t Given current I = 2.0 A and time t = 10 minutes = 10 60 seconds = 600 seconds.Q = 2.0 A 600 s = 1200 CoulombsStep 2: Determine the moles of copper deposited n .Copper has a valency of +2 Cu , which means that 2 moles of electrons are required to deposit 1 mole of copper. The relationship between the charge, moles of electrons, and the Faraday constant is given by:Q = n F zWhere Q is the total charge, n is the moles of copper deposited, F is the Faraday constant, and z is the valency of copper 2 in this case .Rearranging the equation to solve for n:n = Q / F z We know the value of Q 1200 Coulombs and z 2 , but we don't know the value of F yet. However, we can use the known value of the Faraday constant approximately 96485 C/mol to calculate the moles of copper deposited:n = 1200 C / 96485 C/mol 2 n 0.0062 molesStep 3: Use the moles of copper and the total charge to calculate the Faraday constant.Now that we have the moles of copper deposited, we can use this value to determine the Faraday constant:F = Q / n z F = 1200 C / 0.0062 moles 2 F 96774 C/molThe calculated value of the Faraday constant is approximately 96774 C/mol, which is close to the known value of 96485 C/mol. The slight difference could be due to experimental errors or rounding in the calculations.