# What volume of oxygen is required to obtain sulfur (IV) oxide from hydrogen sulfide with a volume of 89.6 liters?

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 = 89.6 / 22.4 = 4 mol;

To oxidize such an amount of hydrogen sulfide, 6 moles of oxygen are needed.

Let’s calculate its volume.

To do this, multiply the amount of substance by the volume of 1 mole of gas (22.4 liters).

V O2 = 6 x 22.4 = 134.4 liters; One of the components of a person's success in our time is receiving modern high-quality education, mastering the knowledge, skills and abilities necessary for life in society. A person today needs to study almost all his life, mastering everything new and new, acquiring the necessary professional qualities.