URGENT! chemistry- percentage yield

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?

  1. 👍 0
  2. 👎 0
  3. 👁 335
  1. 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

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    A 46.9 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 11.6 grams. What was the percent iron in the sample of ore? Answer

  2. Chemistry

    A SAMPLE OF ANTIMONY, Ar=121.8, WAS ANALYSED AND WAS FOUND TO CONSIST OF 60% OF 121Sb AND ONE OTHER ISOTOPE. DETERMINE THE MASS NUMBER OF THE OTHER ISOTOPE IN THE SAMPLE OF ANTIMONY. please help I'm really stuck,

  3. Chemisrty

    A 38 g sample of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 11.1 g. What was the mass of iron in the sample of ore?

  4. Chimestry

    (Iron ore is impure Fe_2O_3. When Fe_2O_3 is heated with an excess of carbon (coke), metallic iron and carbon monoxide gas are produced. From a sample of ore weighing 950kg , 533kg of pure iron is obtained). What is the mass

  1. chemistry

    A 1.362 g sample of an iron ore that contained Fe_3O_4 was dissolved in acid and all the iron was reduced to Fe^2+. the solution was then acidified with H_2SO_4 and titrated with 39.42 mL of 0.0281 M KMnO_4 , which oxidized the

  2. AP Chem

    An ore contains Fe3O4 and no other iron. The iron in a 51-gram sample of the ore is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 21.9 g. What was the mass of Fe3O4 in the sample of

  3. AP chemistry

    A 28 g sample of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 19.5 g. What was the mass of iron in the sample of ore?

  4. AP Chemistry

    An ore contains Fe3O4 and no other iron. The iron in a 36.5-gram sample of the ore is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 26 g. What was the mass of Fe3O4 in the sample of

  1. Chemistry

    The following equilibrium was studied by analyzing the equilibrium mixture for the amount of H2S produced. Sb2S3(solid)+3H2(gas)2Sb(solid)+3H2S(solid) A vessel whose volume is 2.5L is filled with 0.0100 mole of

  2. Chemistry

    A sample of an oxide of antimony (Sb) contained 51.5 g of antimony combined with 16.9 g of oxygen. What is the simplest formula for the oxide?

  3. AP Chemistry

    A 33.8 g sample of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 20.7 g. What was the mass of iron in the sample of ore?

  4. Chemistry

    1.630 g of iron ore is dissolved in an acidic solution. This solution is titrated to a pink endpoint with 27.15 mL of a 0.020 M KMnO4 solution. a. How many moles of MnO4- ions were consumed? b. How many moles of Fe2+ were in the

You can view more similar questions or ask a new question.