If a furnace burns an amount of coal containing 198.20 g of FeS2, how much SO2 (an air pollutant) is produced?

Question

Select one:

a. 211.7

b. 52.92

c. 590.8

d. 582.1

Answer 1

It looks like this problem requires a balanced equation. To balance this equation means to have an identical number of atoms on each side, for each element (Fe, S, O) in the equation. Without knowing exactly what is the balanced equation, you might need to make an assumption or two.

Did this problem come with hints or additional information?

Answer 2

Combustion of FeS₂. iron (IV)sulfide reacts with oxygen gas to form iron III oxide and sulfur dioxide gas.

Write a balanced equation:

4FeS₂ + 11O₂ ==> 2Fe₂O₃ + 8SO₂

moles FeS₂ used = 198.20 g x 1 mol/119.975 g = 1.6520 moles

moles SO₂ formed = 1.6520 moles FeS₂ x 8 moles SO₂/4 moles FeS₂ = 6.6080 moles

mass SO2 formed = 6.6080 moles X64.063 g/mol = 427.08 g (5 sig. figs.)