# How much oxygen is needed for the complete combustion of 51 g of hydrogen sulfide H2S

How much oxygen is needed for the complete combustion of 51 g of hydrogen sulfide H2S if this produces sulfur oxide 4 and water?

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, divide its weight by the weight of 1 mole of hydrogen sulfide.

M H2S = 2 +32 = 34 grams / mol; N H2S = 51/34 = 1.5 mol;

To oxidize such an amount of hydrogen sulfide, you need 1.5 x 1.5 = 2.25 mol of oxygen.

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 = 2.25 x 22.4 = 50.4 liters;

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