In a Metallurgical Process the Mineral Pyrite,FeS₂,is Roasted in Air $\to$

question 133

Essay

In a metallurgical process the mineral pyrite,FeS₂,is roasted in air:
FeS₂ + O₂ $\to$ Fe₂O₃ + SO₂
The SO₂ is then converted into H₂SO₄ in the following reactions:
2SO₂ + O₂ $\to$ 2SO₃
SO₃ + H₂SO₄ $\to$ H₂S₂O₇
H₂S₂O₇ + H₂O $\to$ 2H₂SO₄
Assuming the mineral is 24.0% FeS₂ and the remainder is inert,what mass of H₂SO₄ is produced if 155 g of the mineral is used?

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