What is the limiting reagent? Calculate the theoretical yield of iron(3)oxide(Fe2O3)? The reaction produces 6.14g of oxide. What’s the percent yield of the reaction? (See Description)

Question

Iron reacts with oxygen at high temperatures to form iron(III) oxide.

4 Fe(s) + 3O2(g) = 2 Fe2O3g (s)

Suppose 22.8 g of iron (Fe) is reacted with 28.4 g of oxygen (O2)

Answer 1

4 Fe(s) + 3O₂₍g) = 2 Fe₂O₃ (s) ... balanced equation

Limiting reactant:

22.8 g Fe x 1 mol Fe / 55.85 g = 0.408 mols Fe (÷4->0.10)

28.4 g O₂ x 1 mol O₂ / 32 g = 0.888 mols O₂ (÷3->0.3)

Fe is limiting (0.10 is less than 0.3)

Theoretical yield of Fe₂O₃ = 0.408 mols Fe x 2 mols Fe₂O₃ / 4 mols Fe x 160 g/mol Fe₂O₃ = 32.6 g Fe₂O₃

Percent yield = actual yield/theoretical yield (x100%) = 6.14 g / 32.6 g (x100%) = 18.8% yield