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When 0.422 g of a phosphorus is burned 0.967 g of a white oxide is obtained What is the empirical formula of the oxide and also the balanced equation for the reaction of phosphorus and o2 from the EF?
Wiki User
∙ 14y ago
I think i have the first part right
First determine the weight of the oxygen that combined, then get moles of P & O, and determine the ratio in whole numbers
Moles of P 0.422/30.97g/m= .0136 moles of P
moles of 02 (0.967-0.422)g/16.00 g/mole = .0340 of O
0/P= .0340/.0136 = 2.5
This part im not sure i think in to put it in to the correct forumula it would be 2P05
Wiki User
∙ 14y ago
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