Xenon can be made to react with fluorine gas to produce xenon tetrafluoride. If 16.30 g of xenon is used, what
mass of fluorine, in grams, is needed to react completely with the xenon?
chemical
Let's write out the chemical reaction
F2 + Xe ⇒ XeF4
let's balance this reaction
2 F2 + Xe ⇒ XeF4
Xenon and Flouride chem reaction
molecular weights
Xe = 131.29 g/mole
F = 18.99 g/mole
F2 = 37.98 g/mole
reactions
16.30 g Xe
(1 mole Xe)/(131.29 g Xe)
(2 moles F2)/(1 mole Xe)
(37.98 g F2)/(1 moles F2)
= 9.43 g F2
9.43 g F2 are needed to completely react with 16.30 g of Xe