Question

Sulfuric acid is produced by the following process:
    FeS2 + O2 →    Fe2O3 +   SO2
   SO2 + O2 →    SO3
   SO3 + H2O → H2SO4
Balance each reaction and then write a balanced net reaction. How many moles of O2 and H2O will be needed when 10.0 kg of FeS2 reacts completely?

Answer 1

Balanced chemical equation:

A balanced chemical equation is an equation that contains same number of atoms as well as of each element on each side of reaction

Sulfuric acid is produced by the following process:

    4 FeS2 + 11 O2 ---- >   2 Fe2O3 + 8 SO2

   8 [SO2 +1/2 O2 ---- >    SO3] = 8SO2 + 4 O2 ---- >   8 SO3

     8 SO3 +8 H2O ---- > 8 H2SO4

    4 FeS2 + 11 O2 ---- >   2 Fe2O3 + 8 SO2

        8SO2 + 4O2 ---- >   8 SO3

        8 SO3 +8 H2O ---- > 8 H2SO4

4FeS2 + 15O2 + 8H2O ---> 2Fe2O3 + 8H2SO4

Given that 10.0 kg FeS2

1000 g = 1.0 kg

Thus 10.0 kg = 10,000 g FeS2

Now number of moles FeS2= amount in g/ molar mass

= 10,000 g FeS2 /119.965 g/mol

= 83.36 moles FeS2

Now calculates the moles of O2 and H2O which will be needed when 10.0 kg of FeS2 reacts completely as follows:

Moles O2 = 83.36 moles FeS2* 15 moles O2 / 4.00 moles FeS2

= 312.6 moles O2

Moles H2O = 83.36 moles FeS2* 8 moles H2O / 4.00 moles FeS2

= 166.72 moles H2O