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Gas laws question

  1. May 14, 2007 #1
    1. The problem statement, all variables and given/known data
    What is the resulting pressure when the quantities of gases listed below
    are mixed and placed in a 12 L vessel at constant temperature?
    4.0 L Ne measured @ 2.0 atm
    2.0 L He measured @ 3.0 atm
    2.0 L Ar measured @ 5.0 atm

    2. Relevant equations
    P1V1=P2V2

    3. The attempt at a solution
    the answer is 2.0 atm.and i have no clue how they figured that out.
    because i tried to do it by the above equation. and that definitely did not work out.and then i tried adding up the initial volumes:8 L and the initial temperatures:10 atm.and that didn't work either.so basically;i need helpp.
    and hopefully.before tuesday morning.because that's when my ap chem test is. which is why you see me here posting all these questions.

    thanks a lot physicsforum people.you guys seriously save my life these days :redface:
     
    Last edited: May 14, 2007
  2. jcsd
  3. May 14, 2007 #2
    One method: calculate the number of mole of each component, add up, use the perfect gas law for the desired volume.

    Second method: convert all components as volumes for 1 atm, add up the volumes still at 1 atm, compress to the desired volume. (this method is the same as the previous one, but moles are replaced by "standard volume").
     
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