The mass of oxygen required for complete combustion of 67.2 O hydrogen sulfide to SO2 is …

The oxidation reaction of hydrogen sulfide is described by the following chemical reaction equation.

2H2S + 3O2 = 2H2O + 2SO2;

2 moles of hydrogen sulfide reacts with 3 moles of oxygen. In this case, 2 mol of water and 2 mol of sulfur dioxide are synthesized.

Let’s calculate the chemical amount of hydrogen sulfide.

To do this, we divide its volume by the volume of 1 mole of hydrogen sulfide.

N H2S = 67.2 / 22.4 = 3 mol;

To oxidize such an amount of hydrogen sulfide, you need 3 x 1.5 = 4.5 mol of oxygen.

Let’s calculate its weight.

To do this, multiply the amount of substance by the weight of 1 mole of gas.

M O2 = 16 x 2 = 32 grams / mol;

m O2 = 32 x 4.5 = 144 liters;