What is the mass of oxygen required to burn phosphorus with an amount of 2 mol?

The synthesis of phosphorus oxide occurs in accordance with the following chemical reaction equation (CCR):

4P + 5O2 = 2P2O5;

From 2 moles of phosphorus, 1 mole of its oxide is formed (that is, the reaction proceeds in a 2: 1 ratio). In this case, 4 moles of phosphorus react with 5 moles of oxygen.

By the condition of the problem:

N P = 2 mol;

Using the coefficients of the equation, we determine the required amount of oxygen.

To burn such an amount of phosphorus, you will need to take 2 x 5/4 = 2.5 mol of oxygen.

Let’s calculate its weight.

To do this, multiply the chemical (molar) amount of a substance by the weight of 1 mole (its molar weight).

M O2 = 32 grams / mol;

m O2 = 2.5 x 32 = 80 grams;