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9 September, 14:01

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?

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  1. 9 September, 14:07
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    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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