What mass of copper would be formed when a current of 10.0 A is passed through a solution of CuSO4 for 1 hour? [Cu = 63.5; 1F = 96500C]

The mass of copper that would be formed can be calculated using Faraday's law of electrolysis. According to the law, the amount of substance produced at an electrode is directly proportional to the amount of electric charge passed through the electrolyte. Mathematically, the amount of substance produced (in moles) is given by: moles of substance = (electric charge passed) / (Faraday constant * ionic charge) In this case, copper ions (Cu2+) are being reduced at the cathode, so the ionic charge is 2+. The Faraday constant is 96500 C mol-1, which means that one mole of electrons corresponds to a charge of 96500 C. Now, we need to determine the amount of electric charge that is passed through the solution of CuSO4. We are given that a current of 10.0 A is passed through the solution for 1 hour. This means that the total electric charge passed is: electric charge passed = current x time electric charge passed = 10.0 A x 3600 s electric charge passed = 36000 C Substituting the values of electric charge, Faraday constant, and ionic charge into the above equation, we get: moles of Cu = (36000 C) / (96500 C mol-1 x 2) moles of Cu = 0.1869 mol Finally, we can calculate the mass of copper (Cu) that is formed using its molar mass: mass of Cu = moles of Cu x molar mass of Cu mass of Cu = 0.1869 mol x 63.5 g/mol mass of Cu = 11.86 g (rounded to two decimal places) Therefore, the mass of copper that would be formed when a current of 10.0 A is passed through a solution of CuSO4 for 1 hour is 11.86 g. Hence, the correct answer is.