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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