Question

A 50.51g sample of a compound made from phosphorus and chlorine is decomposed.Analysis of the products showed that 11.39 g of phosphorus atoms were produced. What is the empirical formula of the compound?

Answer 1

1) Moles of Phosphorous = mass of phosphorous / molar mass = 11.39 g / 30.98 g mol-1â = 0.3676 moles

2) Moles of Chlorine = (50.51 - 11.39) g / 35.5 g mol-1â = 1.102 moles

Dividing the moles of P and Cl by the smallest number, which is 0.3676, we get the ratio of moles of P : Cl

P = 0.3676 / 0.3676 = 1
Cl = 1.102 / 0.3676 = 3

So the empirical formula is, PCl3.



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