Partial Pressure from decomposition

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SUMMARY

The discussion centers on calculating the partial pressure of nitrogen dioxide (NO2) resulting from the decomposition of dinitrogen pentaoxide (N2O5) in a gas-reaction container. Initially, N2O5 is at a pressure of 130 kPa, and upon decomposition, the total pressure rises to 166 kPa. Utilizing Dalton's Law of Partial Pressure, the relationship between the total pressure and the partial pressures of the gases involved is established, leading to the conclusion that the partial pressure of NO2 can be derived from the change in moles during the reaction.

PREREQUISITES
  • Understanding of Dalton's Law of Partial Pressure
  • Familiarity with gas reaction stoichiometry
  • Knowledge of chemical equilibria concepts
  • Basic skills in manipulating equations involving pressure and mole fractions
NEXT STEPS
  • Study the application of Dalton's Law in gas mixtures
  • Learn about the stoichiometry of gas reactions, particularly decomposition reactions
  • Explore the concept of mole fractions and their relation to partial pressures
  • Investigate the principles of chemical equilibria and how they affect gas reactions
USEFUL FOR

This discussion is beneficial for atmospheric chemists, students studying gas laws, and anyone interested in the principles of chemical reactions and their effects on gas pressures.

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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