What mass of hydrogen sulfide needs to be burned in an excess of oxygen in order to obtain the same volume

What mass of hydrogen sulfide needs to be burned in an excess of oxygen in order to obtain the same volume of sulfur oxide (4), which is formed when burning 800 g of technical sulfur containing 20% of impurities?

The oxidation reaction of sulfur with oxygen is described by the following chemical reaction equation:

S + O2 = SO2;

Let’s find the chemical amount of sulfur. For this purpose, we divide its weight by its molar mass.

M S = 32 grams / mol;

N S = 800 x 0.8 / 32 = 20 mol;

When 20 mol of sulfur is burned, 20 mol of sulfur dioxide will be synthesized.

The oxidation reaction of hydrogen sulfide with oxygen proceeds in accordance with the following chemical equation:

H2S + 3/2 O2 = H2O + SO2;

To get 20 mol of sulfur dioxide by burning hydrogen sulfide, you need to take the same amount of hydrogen sulfide.

Let’s determine its weight. For this For this purpose, we multiply the amount of the substance by its molar mass.

M H2S = 2 + 32 = 34 grams / mol;

m H2S = 20 x 34 = 680 grams;