White phosphorus, p4, spontaneously bursts into flame when exposed to oxygen. if 6.500 g of white phosphorus reacts with oxygen to form 11.54 g of a phosphorus oxide, what is the empirical formula of this oxide?

Empirical formula for the oxide is P₂O₃

Explanation:

Oxides from P, are:

P₂O; P₂O₃; P₂O₅; P₂O₇; P₄O₆; P₄O₁₀

The reaction is:

P₄  +  3O₂  →  P₄O₆

Ratio between the white phosphorus and the oxide is 1:1

Molar mass P₄ = 123.89 g/m

Mass / Molar mass = mole

6.5 g/ 123.89 g/m = 0.0524 mole P₄

0.0524 mole of P₄O₆ have been formed.

Molar mass P₄O₆  = 219.89 g/m

Mol . molar mass = mass

0.0524 mole . 219.89 g/m = 11.52 g

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