# chemistry

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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.

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