CS2 (s) + 3 O2 (g) → CO2 (g) + 2 SO2 (g)

Using the formula above how many liters of SO2 can be made from 3.1 L of O2 at STP? Round your answer to two decimal places.

2.067 L ≅ 2.07 L.

Explanation:

The balanced equation for the mentioned reaction is:

CS₂ (g) + 3O₂ (g) → CO₂ (g) + 2SO₂ (g),

It is clear that 1.0 mole of CS₂ react with 3.0 mole of O₂ to produce 1.0 mole of CO₂ and 2.0 moles of SO₂.

At STP, 3.6 L of H₂ reacts with (? L) of oxygen gas:

It is known that at STP: every 1.0 mol of any gas occupies 22.4 L.

using cross multiplication:

1.0 mol of O₂ represents → 22.4 L.

? mol of O₂ represents → 3.1 L.

∴ 3.1 L of O₂ represents = (1.0 mol) (3.1 L) / (22.4 L) = 0.1384 mol.

To find the no. of moles of SO₂ produced from 3.1 liters (0.1384 mol) of hydrogen:

Using cross multiplication:

3.0 mol of O₂ produce → 2.0 mol of SO₂, from stichiometry.

0.1384 mol of O₂ produce →? mol of SO₂.

∴ The no. of moles of SO₂ = (2.0 mol) (0.1384 mol) / (3.0 mol) = 0.09227 mol.

Again, using cross multiplication:

1.0 mol of SO₂ represents → 22.4 L, at STP.

0.09227 mol of SO₂ represents →? L.

∴ The no. of liters of SO₂ will be produced = (0.09227 mol) (22.4 L) / (1.0 mol) = 2.067 L ≅ 2.07 L.