Question

Phosphorus forms several compounds with oxygen, including diphosphorus trioxide and diphosphorus pentoxide. A decomposition of a sample of diphosphorus trioxide forms 1.29 g phosphorus to every 1.00 g oxygen. The decomposition of a sample of diphosphorus pentoxide forms 0.775 g phosphorus to every 1.00 g oxygen. Show that these results are consistent with the law of multiple proportions.

Answer 1

Answer:

Results are consistent with law of multiple proportions.

Explanation:

Dalton's law of multiple proportions states that the elements can be combined to form more than one compound and do so in such a way that if we keep the quantity of one element as fixed, the quantity of the other element is added in such a way that they are obtained integer proportions.

Molar mass of oxygen is 16g per mole, molar mass of phosphorus is 31g per mole.

In $P_{2}O_{3}$ the ratio between P and O is $\frac{31gPx2}{16gOx3} = 1.29\frac{gP}{gO}$, that is consistent with the experimental result.

and for $P_{2}O_{5}$ the ratio between P and O is $\frac{31gPx2}{16gOx5}= 0.775\frac{gP}{gO}$ that is also consistent with experimental results. In conclusion we can say that the results obtained are consistent with the law of multiple proportions.