The Claus reactions,shown below,are used to generate elemental sulfur from hydrogen sulfide. 2H₂S + 3O₂ $\to$ 2SO₂ + 2H₂O
SO₂ + 2H₂S $\to$ 3S + 2H₂O
How much sulfur (in grams) is produced from 21.5 grams of O₂?

Question

The Claus reactions,shown below,are used to generate elemental sulfur from hydrogen sulfide. 2H₂S + 3O₂

\to

2SO₂ + 2H₂O
SO₂ + 2H₂S

\to

3S + 2H₂O
How much sulfur (in grams) is produced from 21.5 grams of O₂?

Quizplus · Accepted Answer

First, calculate moles of O₂: 21.5 g / 32.00 g/mol = 0.6719 mol O₂. From the first reaction, 3 mol O₂ produces 2 mol SO₂. From the second reaction, 1 mol SO₂ reacts with 2 mol H₂S to produce 3 mol S. Therefore, 0.6719 mol O₂ produces (0.6719 mol O₂ * 2/3 * 3) = 1.3438 mol S. Convert moles of S to grams: 1.3438 mol * 32.07 g/mol = 43.1 g S.

The Claus Reactions,shown Below,are Used to Generate Elemental Sulfur from Hydrogen