Sulfuric acid may be produced by the following process: 4FeS₂+ 11O₂ $\to$ 2Fe₂O₃ +8SO₂
2SO₂ +O₂ $\to$ 2SO₃
SO₃ + H₂O $\to$ H₂SO₄
How many moles of H₂SO₄ will be produced from 8.41 moles of FeS₂?

Question

Sulfuric acid may be produced by the following process: 4FeS₂+ 11O₂

\to

2Fe₂O₃ +8SO₂
2SO₂ +O₂

\to

2SO₃
SO₃ + H₂O

\to

H₂SO₄
How many moles of H₂SO₄ will be produced from 8.41 moles of FeS₂?

Quizplus · Accepted Answer

The balanced chemical equation shows that for every 4 moles of FeS₂, 1 mole of H₂SO₄ is produced. Thus, we can use a mole ratio to calculate the number of moles of H₂SO₄ produced: 8.41 moles FeS₂ x (1 mole H₂SO₄ / 4 moles FeS₂) = 2.10 moles H₂SO₄ Therefore, the answer is (E) 2.10.

Sulfuric Acid May Be Produced by the Following Process: 4FeS2 →\to→

Sulfuric Acid May Be Produced by the Following Process: 4FeS_{2 $\to$}