How many grams of sulfuric acid,H₂SO₄,can be obtained from 400 grams of iron ore if the ore is 80.0% by mass FeS? The reactions involved are given below.
4 FeS + 7O₂ → 2 Fe₂O₃ + 4 SO₂
2 SO₂ + O₂ → 2 SO₃
SO₃ + H₂O → H₂SO₄

Question

Quizplus · Accepted Answer

First, calculate the mass of FeS in the ore: 400 g * 80% = 320 g FeS. The molar mass of FeS is approximately 88 g/mol, so there are about 320 g / 88 g/mol = 3.64 mol of FeS. From the first reaction, 4 mol of FeS produce 4 mol of SO2, so 3.64 mol of FeS will produce approximately 3.64 mol of SO2. Following through the reactions, these 3.64 mol of SO2 will eventually yield 3.64 mol of H2SO4. The molar mass of H2SO4 is approximately 98 g/mol, so the mass of H2SO4 produced is 3.64 mol * 98 g/mol = 356.72 g, which rounds to 357 g.

How Many Grams of Sulfuric Acid,H2SO4,can Be Obtained from 400

How Many Grams of Sulfuric Acid,H₂SO₄,can Be Obtained from 400