If 112 g of iron (Fe) combines with 24 g of oxygen (o2) how much iron oxide is formed

There are three different oxides of iron: FeO, Fe2O3 (hematite), and Fe3O4 (magnetite). Assuming that the iron oxide formed in this problem is Fe2O3, which is the most common form of iron oxide, the calculations are as follows:

Balanced chemical equation:

4Fe + 3O2 - - > 2Fe2O3

i 2 0.75 0

c 1 0.75 0.5

e 1 0 0.5

Moles Fe = 112g / 55.845 = 2

Moles O2 = 24/32 = 0.75

The reaction, with an excess of 1 mol Fe, produced 0.5 moles or 0.5 moles (159.69g/mol) = 79.845 grams of Fe2O3.