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Jef123

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**1. 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. 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?**

**2. Molecular formula = XeO**

_{4}**3. I used the ideal gas law formula PV = nRT. I know that the moles (n), gas constant (R), and volume (V) are constant, so I can solve for the new pressure using the equation P**

_{1}/T_{1}= P_{2}/T_{2}. Rearranging to solve for P_{2}= 0.313 atmApparently 0.313 atm is the partial pressure for Xenon and 0.626 atm is the partial pressure for oxygen. I know that when the temperature is increased that the compound breaks into its constituent elements (i.e. Xe and 2O

_{2}) but what I do not understand is why would the equation I used to solve for pressure give me the partial pressure of xenon? I thought that 0.313 atm would be the total pressure of both gases in the vessel?