How much oxygen is consumed for the combustion of phosphorus if phosphorus (V)

How much oxygen is consumed for the combustion of phosphorus if phosphorus (V) oxide with a mass of 56.8 g is formed?

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

4P + 5O2 = 2P2O5;

4 phosphorus atoms interact with 5 oxygen molecules. During the reaction, 2 molecules of pentavalent phosphorus oxide are synthesized.

Let’s calculate the chemical amount of a substance contained in phosphorus oxide weighing 56.8 grams.

M P2O5 = 31 x 2 + 16 x 5 = 142 grams / mol;

N P2 O5 = 56.8 / 142 = 0.4 mol;

To synthesize such an amount of oxide, it is necessary to take 0.4 / 2 x 5 = 1 mole of oxygen.

Let’s calculate its volume.

To do this, multiply the amount of oxygen by the volume of 1 mole of gas.

1 mole of ideal gas fills a volume of 22.4 liters under normal conditions.

V O2 = 1 x 22.4 = 22.4 liters;