The mass of oxygen that would be required to produce enough CO, which completely reduces 1.6 kg Fe2O3  is ___ ?

C+12O2→CO Fe2O3+3CO→2Fe+3CO2Gram molecular weight of Fe2O3 is (2×56)+(3×16)=160 g per mole Fe2O3+3CO→2Fe+3CO2 160 g of Fe2O3 Need 84 g of CO for complete reduction   Then 1.6×103 g of Fe2O3 require 1.6×103×84160=840 g of CO C+12O2→CO 16 Gram of oxygen is required to produce (12+16)=28g of CO  Then amount of oxygen required to produce 840 g of CO is 840×1628=480 g