Question

Sulfur is used in the production of vulcanized rubber, detergents, dyes, pharmaceuticals, insecticides, and many other substances. The final step in the Claus method for making sulfur is SO2 (8)+2HS (8)- 3S (s) + 2H2O () a. What minimum volume of sulfur dioxide at STP would be necessary to produce 82.5 kg of sulfur? V.7So roS82.skys 1000g rele 1 K 32.oug

Answer 1

The balanced equation,

SO₂ (g) + 2 H₂S (g) --------> 3 S (s) + 2 H₂O (l)

Mass of Sulfur = 82.5 kg = 82.5 * 1000 = 82500 g

Number of moles of sulfur = 82500 g/(32.06 g/mol) = 2573.3 mol

According to balanced equation,

3 moles of S is produced from 1 mole of SO₂

So, 2578.125 mol of S would be produced from 2573.3 mol * 1/3 = 857.7667 mol of SO₂

Number of moles of SO₂ = 857.7667 mol

Temperature = 0 °C = 273.15 K

P = 1 atm

V= nRT/P = 857.7667 mol * 0.0821 L.atm.mol^-1.K^-1. * 273.15 K/1 atm =19235.95 L

Volume of SO₂ = 19236 L