[itsme03]

the problem states:
a compound of chlorine and fluorine, ClF_n, reacts at about 75 degrees C with uranium metal to produce uranium hexafluoride, UF₆, and chlorine monofluoride, CIF_(g). a quantity of uranium produced 3.53 g UF₆ and 343 mL ClF at 75 degrees C and 2.50 atm. what is the formula (n) of the compound?

i got the moles of ClF_(g) = 0.30 mol
and the moles of UF₆ = 0.01mol

but how do i get the formula of ClF_n after that? i know I'm supposed to get the mol of F from the two products, but how?? i really want to understand this

the answers supposed to be ClF₃.

[Borek]

Calculate total moles of F and Cl in products.