An electrolytic cell produces aluminum from Al2O3 at the rate of ten kilograms a dayAssuming a yield of 100%a) how many moles of electrons must pass through the cell in one day?c) how many moles of oxygen (O2) are being produced simultaneously? I understand that for part a, you start with 5kg, and that you use dimensional analysis, but what I'm stuck on is the stoichometry for the electrons (3 for Al, 4 for O, 7 for both, or 12 for canceling out?) and if you go from kg to g (molar mass) of Al2O3.Part c is a mystery to me at the moment.
