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% FeS₂and the remainder is inert,what mass of H₂SO₄ is produced if 155 g of the mineral is used?

Question

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% FeS₂and the remainder is inert,what mass of H₂SO₄ is produced if 155 g of the mineral is used?

Quizplus · Accepted Answer

The Answer of 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% FeS₂and the remainder is inert,what mass of H₂SO₄ is produced if 155 g of the mineral is used?

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

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