When the vessel and its contents are warmed to 100 °c, q decomposes into its constituent elements. what is the total pressure, and what are the partial pressures of xenon and oxygen in the container?

The question is incomplete, but here is a similar question with complete details ; Gaseous compound Q contains only xenon and oxygen . When 0.100 g of Q is placed in a 50.0 mL steel vessel at 0 °C, the pressure is 0.229 atm. (a) What is the molar mass of Q (b) When the vessel and its contents are warmed to 100 °C, Q decomposes into its constituent elements . What is the total pressure , and what are the partial pressures of Xenon and Oxygen

Explanation:

The step by step calculations is as shown in the attached file.

It should be noted that what was applied is

The Ideal gas equation PV = nRT Daltons law of partial pressure which states that in a mixture of gases, the total pressure exerted is equal to the sum of the individual partial pressures of the gases at constant temperature. It should be noted that the total pressure of the gases can be gotten by applying pressures law at constant volumeP1/P2 = T1/T2It should also be noted that Partial pressure = Total pressure x Mole fraction

Mri is one what are your options anyway ?

True i’m pretty sure