Question

The question says: when .422 g of phosphorus is burned, .967 g of a white oxide is obtained. Determine the empirical formula of the oxide.

I did the calculations and got that there would be 1 mole Phosphorus and 4.29 mol Oxygen. To get the empirical formula, I would need to get them to whole numbers, right? What would my whole numbers be?
Nevermind, I think I've figured out what I was doing wrong!!

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