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Gaseous xenon fluoride can be prepared by shining light on a mixture of Xe and $F_{2}$ gases. Assume that xenon gas was added to a 0.25L flask until its pressure was 0.12 atm at ${0.0}^{o} C$ . Fluorine gas was then added until the total pressure becomes 0.36 atm at ${0.0}^{o} C$ . After the reaction was complete, the xenon had been consumed completely and the total pressure of the gases remaining in the flask was still 0.24atm at $0^{o} C$ . The formula of compound prepared from Xe and $F_{2}$ is $X e F_{2 n}$ then $n$ is_____

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Detailed Solution

$Xe (g) + n F_{2} (g) \to X e F_{2 n} (g) I n i t i a l 0.12 0.24 0 F i n a l 0 0.24 - 0.12 n 0.12 0.36 - 0.12 n = 0.24 \Rightarrow n = 1$

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