# How much oxygen is required to completely burn 2 moles of phosphorus? What mass of phosphorus

How much oxygen is required to completely burn 2 moles of phosphorus? What mass of phosphorus (V) oxide is formed in this case?

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.

It is required to burn 2 moles of phosphorus.

To burn this amount of phosphorus, 2 x 5/4 = 2.5 mol of oxygen will be required.

Let’s calculate its volume.

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

The required volume of oxygen will be:

V O2 = 2.5 x 22.4 = 56 liters;

From this amount of phosphorus, it is possible to synthesize 2/2 = 1 mol of its oxide.

Let’s find its weight.

To do this, we multiply the amount of the substance by its molar mass.

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

m P2O5 = 142 x 1 = 142 grams;

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