posted by Anonymous .
Sb2S3(s) + 3 Fe(s) 2 Sb(s) + 3 FeS(s)
When 14.7 g Sb2S3 reacts with an excess of Fe, 9.84 g Sb is produced. What is the percent yield of this reaction?
Follow the steps in this example stoichiometry problem. This will give you the theoretical yield. Then percent yield = (actual yield/theoretical yield)*100 = ?