Post a New Question

chemistry

posted by on .

In an experiement 23.4 g of iron sulphide are added to excess oxygen and 16.5 grams of iron (III) oxide, Fe2O3 are produced the balanced equation for the reaction is 4FeS + 7O2 -- 2Fe2O3 + 2SO2
Calculate the percent yield of iron oxide in the experiement

  • chemistry - ,

    Write and balanced the equation which you have done (wrong) but I corrected it.(You probably just made a typo.)
    4FeS + 7O2 ==> 2Fe2O3 + 4SO2

    2. Convert 23.4 g FeS to moles. moles = grams/molar mass

    3. Using the coefficients in the balanced equation, convert moles FeS to moles Fe2O3.

    4. Now convert moles Fe2O3 to grams. g = moles x molar mass. This is the theoretical yield.

    5. %yield = (actual yield/theoretical yield)*100 = ??

  • chemistry - ,

    quation 2 above
    mole=GM/MM
    =23.4/84
    =0.278571
    =0.21mol.

Answer This Question

First Name:
School Subject:
Answer:

Related Questions

More Related Questions

Post a New Question