An electrolytic cell produces aluminum from Al2O3 at the rate of ten kilograms a day.?

Dimensional Analysis?? This is a question of Electrochemistry.. From Faraday's first law in this domain, Mass of Aluminium produced = Equivelant mass of source( Al2O3 ) / Charge on a mole of electrons x Amount of electricity consumed( quantity of charge ).. Eq. mass of Al2O3 = Molecular mass / no. of electrons transferred during all redox reactions involved per mole of Al2O3 .. Al2O3 --> 2Al(3+) + 3O(2-).. So, 6 electrons have been transferred.. So, mass of Al = 10000 grams = 102/(6 grams x 96500 Coulomb ) x Q Coulomb.. So, Q comes out to be about 56765160 .. Using Faraday's first law again, calculate the amount of O2 produced yourself