Question

Xenon fluoride can be prepared by heating a mixture of Xe and F2 gases to a high temperature in a pressure-proof container. Assume that xenon gas was added to a 0.25 liter container until its pressure reached 0.12 atm at 0.0°C. Fluorine gas was then added until the total pressure reached 0.72 atm at 0.0°C. After the reaction was complete, the xenon was consumed completely, and the pressure of the F2 remaining in the container was 0.36 atm at 0.0°C. What is the empirical formula of the xenon fluoride?

Answer 1

Partial pressure of Xe is 0.12 atm.

Total pressure before reaction is 0.72 atm.

Partial pressure of F2 before reaction = 0.72-12=0.60 atm.

Partial pressure of F2 after reaction = 0.36 atm.

Partial pressure of F2 that consumed during reaction = 0.60-0.36=0.24 atm.

The ratio of partial pressures of Xe and F2 consumed during reaction = 0.12 : 0.24 = 1 : 2

Partial pressure is directly proportional to the number of moles.

Thus, 1 mole of Xe combines with 2 moles of F2 to form XeF4 (xenon tetrafluoride)