A xenon fluoride compound can be prepared by heating a mixture of Xe and F2 to a

Question

A xenon fluoride compound can be prepared by heating a mixture of Xe and F2 to a high temperature in a pressure- proof container made of nickel. Assume that xenon gas was added to a 0.25 L container until its pressure was 0.12 atm. Fluorine gas was then added until the total pressure was 0.72 atm. After the reaction was complete, the xenon had been consumed completely and the pressure of the F2 remaining in the container was 0.36 atm. Note: all pressures were measured at the same constant temperature. What is the empirical formula of the compound prepared from Xe and F2?

Explanation / Answer

P(Xe) reacted = P(Xe) initial = 0.12 atm

P(F2) reacted = P(total) - P(Xe) initial - P(F2) remaining

= 0.72 - 0.12 - 0.36 = 0.24 atm


Ideal gas equation: PV = nRT

At constant T and V => moles n are proportional to P


Moles of Xe : F2 = P(Xe) reacted: P(F2) reacted

= 0.12 : 0.24 = 1 : 2


Since moles of F = 2 x moles of F2:

Moles of Xe : F = 1 : 4


Empirical formula is XeF4

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