The electrolyte concentration was determined as 49.6 g/l Cu2+ at the end of the electrolysis process, which was carried out at a current density of 20 mA/cm2 for 2 hours in a 1L volume of electrolyte containing 50 g/l Cu2+ and 150 g/l H2SO4. In the electrolysis process, 2 stainless steel cathodes and Pb (4% Sb) anode with a surface area of 1000 mm2 were used. Since the cell voltage value measured during the electrolysis process, which is carried out by immersing 50% of the cathode in the electrolyte, is 2.2 V, a) Write down the cathodic and anodic reactions that take place during electrolysis. b) Calculate the current efficiency (%) of the electrolysis process. c) Calculate the specific energy consumption (Ws) of the electrolysis process. Atomic weight of copper: 63.546 g/mol