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March 29, 2017

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

  • Chem problem- 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.

  • Chem problem- percent yield - ,

    Is the percent yield 91.5%?

  • Chemistry Tutor-Verify please - ,

    I got 28.77%

  • Chem problem- percent yield - ,

    Woops! I worked it over and got about 91.5%

    You are right. Sorry.

  • Chem problem- percent yield - ,

    thanks for helping. :)

  • Chem problem- percent yield - ,

    91.5% is correct.

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