A 4.43 gram sample of phosphorus was burned in air to produce 10.15 g of an oxide. What's the empirical formula of this compound?

Answer 1

figure the moles of P in 4.43grams
then in the oxide, you have the same moles of P.

Now you have 10.15g -4.43g O
figure those moles.

You now have the mole ratio of P:O
write the formula PxOy

Answer 2

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