pre ap chem

heating an ore of antimony and iron II sulfide.
Sb2S3+3Fe-->2Sb+3FeS
when 15g Sb2S3 reacts with an excess of Fe, 9.84g Sb is produced. what is the pecent yeild of this reaction?

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  1. Convert 15 g Sb2S3 to mols using mols = g/molar mass.
    Convert mols Sb2S3 to mols mols Sb using the coefficients in the balanced equation.
    Convert mols Sb to grams using g = mols x molar mass. This is the theoretical yield.

    %yield = [(actual yield)/(theoretical yield)]*100
    actual yield is 9.84 g.
    theoretical yield is calculated above.

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