Question

Au ++ 3e → Au The picture above shows a set-up that could be used for electroplating. When the Olympic Games were held in Atlanta, the United States provided gold medals for the athletes. Calculate how many grams of gold would be plated out on a coin, if a current of 3.2 (Amp) is applied for 27 min to an electrolytic cell shown above. The following reaction is occurring: Au3+ + 3 e → Au MW for gold equals 1979 / mol. 1 amp (A) = 1 coulomb/second (C/s) Charge on 1 mol of electrons = 96500 coulombs (C) = 1 faraday (F) Calculate the number of grams plated out. You must take into consideration the number of moles of electrons necessary to reduce each gold ion to gold. Submit Answer Tries 0/45

Answer 1

According to Faraday's law first of electrolysis, the weight of a chemical substance deposited at an electrode is directly proportional to the quantity of electricity passed through the electrolyte.

mathematically, W = z × c × t = Equivalent weight*c*t/96500 where c= current in amperes, t= time in seconds

                              = 197*3.2*27*60/(3*96500) = 3.52 gms

The weight of gold deposited at the electrode = 3.52 gms