posted by Ken .
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?
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.