Consider this reaction: 2Fe (s) + 3S(s) → Fe2S3 (s). Identify the limiting reactant and theoretical yield for the reaction if you start with 1.5 mols of S and 2.0 mols of Fe

Answer 1

1. Limiting Reactant:

3 mol S → 1 mol Fe₂S₃ (based on reaction)

1.5 mol S * (1 mol Fe₂S₃ / 3 mol S) = 0.5 mol Fe₂S₃

2 mol Fe → 1 mol Fe₂S₃ (based on reaction)

2 mol Fe * (1 mol Fe₂S₃ / 2 mol Fe) = 1 mol Fe₂S₃

Since the Sulfur (S) produces less product (Fe₂S₃), it's the limiting reactant.

1. Theoretical yield:

The theoretical yield is the amount of the product (in g) formed from the limiting reagent.

From the previous part, we know the amount of the product (in moles) formed from the

limiting reagent:

0.5 mol Fe₂S₃.

Fe₂S₃ Molar Mass: (207.9 g / mol)

Fe₂S₃ Mass: 0.5 mol Fe₂S₃ * (207.9 g / 1 mol) = 103.95 g Fe₂S₃