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Question:

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

Sb2S3(s) + 3 Fe(s) 2 Sb(s) + 3 FeS(s)When 16.5 g Sb2S3 reacts with an excess of Fe, 9.84 g Sb is produced. What is the percent yield of this reaction?______________%

Answer:

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From the reaction it is know that 1 mole of stibnite (Sb2S3) will react with excess iron to form 2 moles of antimony (Sb). Use the atomic weights to from a ratio to calculated theoretical recovery value. Which would be: 339.68 grams Sb2S3 gives 243.5 grams Sb; So, 16.5 g is X g of antimony. Solve and get X 11.8 grams Sb. But it says that only 9.84 grams is actually recovered! To find the % yield, divide 9.84g (actual result) by the calculated theoretical recovery value of 11.8 g and multiply by 100. Yield (9.84/11.8) * 100 Yield 83.2%

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