The mass of oxygen required for combustion of 67.2 liters of hydrogen sulfide is?

Oxidation of hydrogen sulfide with oxygen is described by the following chemical reaction equation:

H2S + 3/2 O2 = H2O + SO2;

Let’s calculate the molar amount of hydrogen sulfide. To do this, we divide its volume by the volume of 1 mole of gas (which is 22.4 liters).

N H2S = 67.2 / 22.4 = 3 mol;

To burn such an amount of hydrogen sulfide, 3 x 3/2 = 4.5 mol of oxygen will be required.

Let’s calculate its weight.

For this purpose, we multiply the chemical amount of the substance by the molar weight of the substance.

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

m O2 = 4.5 x 32 = 144 grams;