The noxious gas H₂S can be used to remove the acid rain component SO₂ from factory emissions by the Claus Process. What volume of H₂Sin litres at STP will be needed to remove 2.00 kg of SO₂?
2 H₂S₍_g) + SO_2(g) $\rarr$ 3 S_(s) + 2 H₂O_(l)

Question

The noxious gas H₂S can be used to remove the acid rain component SO₂ from factory emissions by the Claus Process. What volume of H₂Sin litres at STP will be needed to remove 2.00 kg of SO₂?
2 H₂S₍_g) + SO_2(g)

\rarr

3 S_(s) + 2 H₂O_(l)

Quizplus · Accepted Answer

The balanced equation shows that 2 moles of H₂S are needed to react with 1 mole of SO₂. The molar mass of SO₂ is 64 g/mol, so 2.00 kg of SO₂ is equal to 2.00 kg / 64 g/mol = 31.25 mol. Therefore, 2 * 31.25 = 62.5 mol of H₂S are needed. At STP, 1 mol of any gas occupies 22.4 L, so 62.5 mol of H₂S will occupy 62.5 mol * 22.4 L/mol = 1400 L.

The Noxious Gas H2S Can Be Used to Remove the Acid

The Noxious Gas H₂S Can Be Used to Remove the Acid