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 15.0 g Sb2S3 reacts with an excess of Fe, 9.84 g Sb is produced. What is the percent yield of this reaction?
Is the percent yield 91.5%?
I got 28.77%
Woops! I worked it over and got about 91.5%
You are right. Sorry.
thanks for helping. :)
91.5% is correct.
To find the percent yield of a reaction, you need to compare the actual yield of the product with the theoretical yield of the product. The actual yield is the amount of product that is actually obtained in the reaction, while the theoretical yield is the maximum amount of product that can be obtained based on stoichiometry.
In this case, the actual yield of antimony (Sb) is given as 9.84 g. We need to determine the theoretical yield of antimony. To do that, we need to calculate the amount of antimony that should be produced based on stoichiometry.
From the balanced chemical equation, we can see that the molar ratio between Sb2S3 and Sb is 1:2. So, if 15.0 g of Sb2S3 is reacted, we can use its molar mass to calculate the number of moles of Sb2S3:
15.0 g Sb2S3 * (1 mol Sb2S3 / molar mass of Sb2S3) = X mol Sb2S3
Next, we can use the molar ratio between Sb2S3 and Sb to calculate the number of moles of Sb:
X mol Sb2S3 * (2 mol Sb / 1 mol Sb2S3) = Y mol Sb
Finally, we can use the molar mass of Sb to convert the moles of Sb to grams:
Y mol Sb * (molar mass of Sb / 1 mol Sb) = theoretical yield of Sb
Now, we can calculate the theoretical yield:
theoretical yield of Sb = Y mol Sb * (molar mass of Sb / 1 mol Sb)
With the theoretical yield and the actual yield, we can calculate the percent yield:
percent yield = (actual yield / theoretical yield) * 100%
Substitute the given values into the equation and solve for the percent yield.
Okay, the formula is Actual Yield/Theortical Yield * 100 = Percent Yield
9.84g Sb is your actual yield
To find your theortical yield, you first have to find the grams of Fe. Then find out which is the limiting reaction. Use the limiting reaction (your theortical yield) and plug it into the formula.