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Heating an ore of antimony (Sb2S3) in the presence of iron yields antimony and iron (II) sulfide.
Sb2S3 + 3 Fe = 2Sb + 3 FeS

When 15g of Sb2S3 reacts with 10g of Fe in the lab 9.84g of Sb is produced.
What is the limiting reactant in this reaction?
What is the theorectical yield of Sb in this reaction?
What is the percent yield?

  • Chemistry -

    mols Sb2S3 = grams/molar mass
    mols Fe = grams/atomic mass

    Convert mols Sb2S3 to mols Sb using the coefficients in the balanced equation.
    Convert mols Fe to mols Sb.
    Most likely mols Fe will not agree which means one of them is wrong. The correct value in limiting reagent problems is ALWAYS the smaller value and the reagent providing that number is the limiting reagent.
    Using the smaller value, convert to g. g = mols Sb x atomic mass Sb. This is the theoretical yield.

    %yield = (actual yield/theor yield)*100 = ?

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