Xenon fluoride can be prepared by heating a mixture of Xe and F2 gases to a high temperature in apressure-proof container. Assume that xenon gas was added to a 0.25 liter container until itspressure reached 0.12 atm at 0.0°C. Fluorine gas was then added until the total pressure reached0.72 atm at 0.0°C. After the reaction was complete, the xenon was consumed completely, and thepressure of the F, remaining in the container was 0.48 atm at 0.0°C. What is the empirical formulaof the xenon fluoride?(MTS 2/2/2018)O XEF3XeF2O XeF4O Xe2FO Xe,FO Xe4F

Answered: Xenon fluoride can be prepared by…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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 F, remaining in the container was 0.48 atm at 0.0°C. What is the empirical formula
of the xenon fluoride?
(MTS 2/2/2018)
O XEF3
XeF2
O XeF4
O Xe2F
O Xe,F
O Xe4F

Expert Solution

Step 1

Dalton's law of partial pressure states that the total pressure equals to the sum of the partial pressure of the individual gases that makes up the mixture.

Thus, Total pressure= Pressure of Xenon + Pressure of Fluoride

P_T= P_Xe+ P_F2

Substituting known,

0.72 = 0.12 + P_F2

Thus, P_F2= 0.60 atm

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