Partial Pressure from decomposition

AI Thread Summary
The discussion revolves around calculating the partial pressure of nitrogen dioxide (NO2) after the decomposition of dinitrogen pentaoxide (N2O5) in a gas-reaction container. The initial pressure of N2O5 is given as 130 kPa, and the total pressure after decomposition is 166 kPa. Participants express confusion over how to relate partial pressure to total pressure without specific volume or temperature data. The conversation emphasizes the need to consider the relationship between total moles of gas and total pressure, suggesting that understanding the decomposition process is crucial for solving the problem. Ultimately, the focus is on applying Dalton's law of partial pressures to find the desired value.
brandon1
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Homework Statement



An atmospheric chemist fills a gas-reaction container with gaseous dinitrogen pentaoxide to a pressure of 130. kPa, and the gas decomposes to nitrogen dioxide and oxygen. What is the partial pressure of nitrogen dioxide, PNO2, (in kPa) when the total pressure is 166 kPa?

Homework Equations



2(N2O5) --> 2(N2O2) + 3(O2)

rate=k[N2O5]

Dalton's law of Partial Pressure

The Attempt at a Solution



P1=130Kpa
P2=166Kpa
PNO2=?

Not sure where to start. There is no mention of this in this chapter. I can't use regular gas laws because I am not given any volumes or temperatures.
 
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Think of an equation that relates partial pressure, mole fraction and total pressure.
 
brandon1 said:
Not sure where to start. There is no mention of this in this chapter.
Looks like "this chapter" is about chemical equilibria.

Assume volume and temperature are constant - call them V, T. Then how is the total pressure related to the total number of moles of gas in the vessel?

What exactly happens to the N2O5 that's put into the vessel? What does this do to the total number of moles?
 

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