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anonymous

  • one year ago

Here is a pic of the question. The question is easy to solve but I need to assume constant pressure to do so. It doesn't mention in the question whether pressure is constant however. But in other questions in the same assignment, pressure is constant. So should it be safe to assume constant pressure or is there a solution I don't see? (Unlikely)

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  1. anonymous
    • one year ago
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    http://tinypic.com/r/2qinsd0/8 The pic can be found at the above link

  2. anonymous
    • one year ago
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    @Abhisar @paki @wio

  3. Abhisar
    • one year ago
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    Where is the question?

  4. anonymous
    • one year ago
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    It's in the picture

  5. anonymous
    • one year ago
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    Question picture link is posted above.

  6. anonymous
    • one year ago
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    @Nnesha @aaronq @zepdrix

  7. anonymous
    • one year ago
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    @texaschic101 @Abhisar

  8. anonymous
    • one year ago
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    @hartnn

  9. anonymous
    • one year ago
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    @Loser66

  10. anonymous
    • one year ago
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    Guys any help/suggestions would be great. I just need some help with making this assumption. The problem itself is easy.

  11. Michele_Laino
    • one year ago
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    I think that the pressure is constant

  12. Michele_Laino
    • one year ago
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    pressure of nitrogen, of course

  13. anonymous
    • one year ago
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    Yeah that's what I wanted to assume as well. This is problem 3, in problem 4 they tell you to take the pressure as constant. That's why I was wondering if it would be a safe assumption. Once I can assume that, all is well.

  14. Michele_Laino
    • one year ago
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    from your picture, I can see that the nitrogen gas makes a free expansion, namely the only pressure against nitrogen is the external pressure, which is constant I think

  15. anonymous
    • one year ago
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    The atmospheric pressure I believe is neglected here and isn't of concern. It's just the heat that is expanding the gas. Since the temperature is increasing, and the temperature is increasing the volume, then it should imply that pressure remains constant.

  16. Michele_Laino
    • one year ago
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    more precisely, I think that the constant pressure has to be considered as an initial hypothesis. Afterthat, if we apply the equation of state ofgases, we can write this: \[\Large {T_{final}} = 2{T_{initial}}\]

  17. Michele_Laino
    • one year ago
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    work \(W\) done by nitrogen gas, is: \[W = {P_1}\left( {{V_2} - {V_1}} \right) = {P_1}\left( {2{V_1} - {V_1}} \right) = {P_1}{V_1}\] where \(P_\,V_\\) are initial pressure and volume of nitrogen, respectively

  18. Michele_Laino
    • one year ago
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    oops... where \(P_1,V_1\) are initial pressure and volume of nitrogen, respectively

  19. anonymous
    • one year ago
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    Yeah all that is trivial. The problem is trivial. The only issue I had was the original assumption. Not looking for a solution, just the help whether I should assume that or not. From what I've read now and what you are saying, that should be the right assumption.

  20. Michele_Laino
    • one year ago
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    ok! :)

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