URGENT! chemistry- percentage yield

posted by .

heating an ore of antimony sulfide in the presence of iron gives th element antimony and iron(2) sulfide. when 15.0 antimony sulfide reacts with an excess of iron, 9.84 g antimony is produced. what is the percent yield of this reaction?

  • URGENT! chemistry- percentage yield -

    You need to calculate the theoretical yield (Y) starting from 15.0 (I presume g) of antimony sulfide. In order to do this you need a balanced equation, so you need to insert symbols and balance:

    iron + antimony sulfide -> antimony + iron(II)sulfide.

    To calculate the theoretical yield find the number of moles of antimony sulfide in 15.0 g.

    15.0 g/(Molar mass of antimony sulfide)

    then calculate the theoretical number of moles of antimony formed using the balanced equation.

    Y (theoretical yield) is then

    Y=moles of antimony x molar mass of antimony.

    percentage yield
    = (9.84 g x 100)/Y

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. pre ap chem

    heating an ore of antimony and iron II sulfide. Sb2S3+3Fe-->2Sb+3FeS when 15g Sb2S3 reacts with an excess of Fe, 9.84g Sb is produced. what is the pecent yeild of this reaction?
  2. chemistry

    How many moles of iron(II)sulfide are produced when 4.38g of Fe reacts with 2.88g of S to produce iron(II)sulfide?
  3. Chem problem- percent yield

    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 …
  4. chemistry

    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 10.9 g Sb2S3 reacts with an excess of Fe, 9.84 g Sb is produced. What is the percent …
  5. chem

    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 10.9 g Sb2S3 reacts with an excess of Fe, 9.84 g Sb is produced. What is the percent …
  6. Chemistry

    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 …
  7. Chemistry

    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 Sb2Sb3 reacts with an excess of Fe, 9.84 g Sb is produced. What is the …
  8. chemistry

    The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 6.35-g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated HCl(aq) and passed over a reducing …
  9. Chemistry

    Heating an ore of antimony (Sb2S3) in the presence of iron yields antimony and iron (II) sulfide. Sb2S3 + 3 Fe = 2Sb + 3 FeS When 15g of Sb2S3 reacts with 10g of Fe in the lab 9.84g of Sb is produced. What is the limiting reactant …
  10. Chemistry

    The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 7.79-g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated HCl(aq) and passed over a reducing …

More Similar Questions