Question

How many grams of

diphosphorus trioxide, P2O3, are
required to produce 10.2 moles of
phosphorous acid, H3PO3?

P2O3 + 3H₂O → 2H3PO3

[?] g P₂O3

Answer 1

Answer: 561 g

Step-by-step explanation:

Answer 2

From the equation, we know that for every 2 moles of phosphorous acid produced, 1 mole of diphosphorus trioxide is consumed.

This means that we need to find the mass of 10.2/2 = 5.1 moles of diphosphorus trioxide.

• The atomic mass of phosphorous is 30.973761998 g/mol.
• The atomic mass of oxygen is 15.9994 g/mol.

So, the formula mass of diphosphorus trioxide is:

• 2(30.973761998)+3(15.9994)=109.945723996 g/mol.

Thus, 5.1 moles have a mass of:

• 5.1(109.945723996), which is about 561 g (to 3 sf)