How many grams of iron (II) oxide can be produced from 3.4 g of iron in this balanced equation? 4Fe + 3O2 🡪 2Fe2O3

Answer 1

How many grams of Fe₂O₃ can be produced from 3.4 g of iron?

4 Fe + 3 O₂ → 2 Fe₂O₃

Let's first find the molar mass of Fe and Fe₂O₃ using the average molecular weights listed on a periodic table:

molar mass of Fe = 55.85 g/mol

molar mass of Fe₂O₃ = 2(55.85 g/mol) + 3(16.00 g/mol) =159.7 g/mol

Next, let's use the following sequence to convert mass of Fe to mass of Fe₂O₃

mass of Fe → moles of Fe → moles of Fe2O3 → mass of Fe2O3

Here's the numerical calculation:

(3.4 g Fe) × (1 mol Fe / 55.85 g Fe) × (2 mol Fe₂O₃ / 4 mol Fe) × (159.7 g Fe₂O₃ / 1 mol Fe₂O₃)

= 4.9 g Fe₂O₃