Question

antimony(III) sulfide is reacted with excess iron. if 175.6 grams of pure antimony is produced what mass of antimony sulfide was required

Answer 1

Answer: -

The chemical formula of Antimony(III) sulfide = Sb₂S₃

Mass of Sb produced = 175.6 g

Molar mass of Sb = 121.76 g /mol

Number of moles of Sb = 175.6g / (121.76 g/mol)

= 1.44 mol

The balanced chemical equation for this reaction is

Sb₂S₃ + 3 Fe → 2 Sb + 3 FeS

From the chemical equation we see

2 mol of Sb is produced from 1 mol of Sb₂S₃

1.44 mol of Sb is produced from $\frac{1 mol Sb2S3 x 1.44 mol Sb}{2 mol of Sb}$

= 0.72 mol of Sb₂S₃

Molar mass of Sb₂S₃ = 2 x 121.76 + 32.06 x 3

= 339.7 g / mol

Mass of Sb₂S₃ = 0.72 mol x 339.7 g/ mol

= 244.58 g

= 244.6 g rounded off to 4 significant figures.