Answer to Question #295016 in General Chemistry for Destiny

Question

Given The following equation : _ Fe+ _ S8 —-> _ FeS

how many grams of iron are needed to react with 13.0 moles of sulfur ?

Answer 1

Solution:

Balanced chemical equation:

8Fe + S₈ → 8FeS

According to stoichiometry:

1 mol of S₈ reacts with 8 mol of Fe

Thus, 13.0 mol of S₈ reacts with:

Moles of Fe = (13.0 mol S₈) × (8 mol Fe / 1 mol S₈) = 104 mol Fe

The molar mass of Fe is 55.845 g/mol

Hence,

Mass of Fe = (104 mol Fe) × (55.845 g Fe / 1 mol Fe) = 5807.88 g Fe = 5808 g Fe

Answer: 5808 grams of iron (Fe) are needed.