Acompound 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

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.

im pretty sure its b