Science/ Chemistry

When 0.422 g of phosphorus is burned, 0.967 g of a white oxide (a compound of phosphorus and oxygen) is obtained.
a. Determine the empirical formula of the oxide.
So for the empirical Formula I got P_2O_5 now it wants me to Write a balanced equation for the reaction of phosphorus and molecular oxygen based on this empirical formula (include states of matter).

I got 4P(s) + 5O2(g) → 2P2O5(s) I don't think this is right can someone please check my work and let me know? Thank you so much!

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  1. P: 30.973762(2)
    O: 15.999(4)
    Ratio of O to P is:
    ((0.967-0.422)/0.422)*(30.973762/15.999) = 2.50

    The empirical formula is correctly derived from the given masses.

    The empirical equation also balances.

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