When 0.422 g of phosphorus is burned, 0.967 of a white oxideis obtained. a. Dete

Question

When 0.422 g of phosphorus is burned, 0.967 of a white oxideis obtained. a. Determine the empirical formula of the oxide. b. Write a balanced equation for the reaction of phosphorusand molecular oxygen on the basis of this empirical formula. When 0.422 g of phosphorus is burned, 0.967 of a white oxideis obtained. a. Determine the empirical formula of the oxide. b. Write a balanced equation for the reaction of phosphorusand molecular oxygen on the basis of this empirical formula.

Explanation / Answer

mass of oxygen = 0.967 g -0.422 g = 0.545 g O moles P = 0.422 g * (1 mol P / 31 g) = 0.0136129032 moles P moles O = 0.545 g *(1 mol O / 16 g) = 0.0340625 mol O divide by 0.0136 0.0136/0.0136 = 1 mol P 0.034/ 0.0136 = 2.50459559 mol O => PO2.5 =>   P2O5 b) 4P + 5O2    =>   2P2O5

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