What mass of iron is required to interact with 2.24 oxygen to form iron oxide (3)?

Given:
m (O2) = 2.24 g
Fe2O3
To find:
m (Fe) -?
Decision
1) 4Fe + 3O2 = 2Fe2O3
2) m1: M1 = m2: M2
Let Fe be x z
3) M1 (Fe) = 56, since 4 moles of iron then 56 x 4 = 224 g / mol
M2 (O2) = 16 X 2 = 32, since 3 moles of oxygen 32 x 3 = 96 g / mol
4) x = (M1 x m2) / M2
x = (224 g / mol x 2.24 g) / 96 g / mol = 5.2 g
Answer: m (Fe) = 5.2 g