Calculate the amount of oxygen that will be consumed in the complete combustion of 8.24 g of phosphorus.

The synthesis reaction of phosphorus oxide is described by the following chemical reaction equation:

4P + 5O2 = 2P2O5;

4 moles of phosphorus react with 5 moles of oxygen. In this reaction, 2 moles of phosphorus oxide are synthesized.

Let’s calculate the chemical amount of a substance in phosphorus with a mass of 15.5 grams.

M P = 31 grams / mol;

N P = 8.24 / 31 = 0.266 mol;

To oxidize such an amount of phosphorus, 0.266 x 5/4 = 0.3325 mol of oxygen is required.

Let’s define its volume.

Under normal conditions, 1 mole of ideal gas assumes a volume of 22.4 liters.

The required volume of oxygen will be:

V O2 = 0.3325 x 22.4 = 7.448 liters;