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 * 0.80 = 320 g FeS. The molar mass of FeS is 87.91 g/mol, so moles of FeS = 320 g / 87.91 g/mol = 3.64 mol. From the first reaction, 4 mol FeS produces 4 mol SO2, so 3.64 mol FeS produces 3.64 mol SO2. From the second reaction, 2 mol SO2 produces 2 mol SO3, so 3.64 mol SO2 produces 3.64 mol SO3. From the third reaction, 1 mol SO3 produces 1 mol H2SO4, so 3.64 mol SO3 produces 3.64 mol H2SO4. The molar mass of H2SO4 is 98.08 g/mol, so mass of H2SO4 = 3.64 mol * 98.08 g/mol = 357 g.

How Many Grams of Sulfuric Acid, H2SO4, Can Be Obtained

How Many Grams of Sulfuric Acid, H₂SO₄, Can Be Obtained