A compound containing xenon and fluorine was prepared by shining sunlight on a mixture of xe (0.339 g) and excess f2 gas. if you isolate 0.437 g of the new compound, what is its empirical formula

Question

Chemistry

Paula Holden

2 February, 00:52

A compound containing xenon and fluorine was prepared by shining sunlight on a mixture of xe (0.339 g) and excess f2 gas. if you isolate 0.437 g of the new compound, what is its empirical formula

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Hubbard · Answer 1

Compound contains Xenon and fluorine

To find the empirical formula we have to find the ratio of Fluorine to Xenon from finding the moles

Moles Xe = 0.339 g / 131.29 g/mol = 0.00258

Moles F = 0.437 - 0.339/18.9984 g/mol = 0.098/18.9984 = 0.005159

By dividing moles of F by moles of Xe, we get

0.005159/0.00258 = 2

So, XeF2 is the empirical formula.