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Isobaric compression from isotherm to adiabat

  1. Sep 1, 2012 #1
    1. The problem statement, all variables and given/known data

    The figure(Figure 1) shows a thermodynamic process followed by 150 mg of helium. Determine the pressure (in atm) at points 1, 2, and 3. Determine the temperature (in °C) at points 1, 2, and 3.

    http://imgur.com/B7lwQ

    n=.0375 mol
    P1=3 atm
    P2=1 atm
    T1=971.85 k
    T2=971.85 k
    V1=1000 cm^3
    V2=V3=3000 cm^3

    2. Relevant equations

    PV=nRT


    3. The attempt at a solution

    I'm only on the pressure part right now. From the given chart P1=3 atm. I used PV=nRT, and got that T1 and T2 are 971.85 K. With that, I used ideal gas law again to get that P2=1 atm. However, I don't know how to get the pressure at point 3 since I don't know the temperature at that point. It looks like it goes through an isobaric compression from the isotherm to the adiabat to me. Any help is appreciated.

    (303000)(.001)=(.0375)(8.314)T, T1=T2=971.85 K

    P(.003)=(.0375)(8.314)(971.85), P2=1 atm
     
    Last edited: Sep 1, 2012
  2. jcsd
  3. Sep 1, 2012 #2

    rock.freak667

    User Avatar
    Homework Helper

    From 1 to 3, the He goes through an adiabatic process such that

    PVγ= constant

    So you will have to use this to get P3
     
  4. Sep 1, 2012 #3
    Ok, I get the PVγ, where γ=5/3 since its a monatomic gas, but what exactly is the constant? Is that supposed to be nR?
     
  5. Sep 1, 2012 #4
    Ok, I think I got it. So it would be P2V2γ=P1V1γ and then just solve for P2
     
  6. Sep 1, 2012 #5
    Thank you for your help!
     
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