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Help with Thermodynamics and Gas Law

  1. Jan 29, 2016 #1
    THE PROBLEM:
    A steam engine's boiler completely converts 2638 g of water at 83.7 °C to steam at 195.4 °C. The steam, at a constant pressure of 3.28 Pa, expands by pushing a piston of radius 9.4 cm a distance of 8.3 cm. What is the change in internal energy of the water-steam system?


    MY WORK:
    First I know Change In Internal Energy = Heat - Work
    So I found heat using MC Delta T and Heat of Vaporization. I got 6665124.107 J.
    Then I found work.
    Change in Volume = Area * Distance
    So in this case it's Pi R2 D or (.094m2)(pi)(.083m) which is .002304m3
    Then Work = Change in Volume * Pressure
    3.8 pascals* .002304m3 = .008755 J
    Change in internal energy = 6665124.107 J - .008755 J = 6665124.098J

    BUT THAT'S WRONG AND I DON'T KNOW WHAT I AM DOING
     
  2. jcsd
  3. Jan 29, 2016 #2
    Something seems very unusual about this problem statement. Is this the exact wording. That 3.28 Pa is very suspect.

    Are you supposed to be using the steam tables for this?
     
  4. Jan 29, 2016 #3
    yes this is the exact wording and I believe so
     
  5. Jan 29, 2016 #4
    Sorry. I'm not able to make sense out of the problem statement. Maybe someone else can figure it out.
     
  6. Jan 29, 2016 #5

    SteamKing

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    A pressure of 3.28 Pa absolute is a pretty strong vacuum, and even a gauge pressure of 3.28 Pa is essentially atmospheric. From a practical standpoint, this figure is in error.
    A pressure of 1 Pa is created by a dollar bill resting on a flat surface. Atmospheric pressure is 101,325 Pa.

    When you say you found the heat added to the water by using MC delta T and Heat of Vaporization, how did you calculate the heat added to the steam after it has supposedly been turned to vapor? This is where steam tables come in handy, but only if you know the pressure.
     
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