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Heating an ore of antimony (Sb2S3) in the presence of iron gives the element antimony and iron(II) sulfide.

Sb2S3(s) + 3Fe(s) ==> 2Sb(s) + 3FeS(s)

When 15.0g Sb2S3 reacts with an excess of Fe, 9.84g Sb is produced. What is the percent yield of this reaction?

  • Chemistry - ,

    1. You have the equation.
    2. Convert 15.0 g Sb2S3 to moles. moles = grams/molar mass.

    3. Using the coefficients in the balanced equation, convert moles Sb2S3 to moles Sb.

    4. Now convert moles Sb to grams. g = moles x molar mass. This is the theoretical yield.

    5. %yield = (actual yield/theoretical yield)*100 = ??
    The problem states that 9.84 g is the actual yield.

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