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Calculation of variation of entropy knowing state's equation

  1. Jan 25, 2012 #1
    1. The problem statement, all variables and given/known data

    A sample of 1.00 mol of an ideal diatomic gas, initially at pressure P and volume V, expands until it has a pressure of 2P and a volume of 2V. What's the entropy change in the gas on this process?

    2. Relevant equations

    2nd Maxwell relation: 7edca29d9b641071f66f0bf13db5aeb8.png

    4th Maxwell relation:
    4679c4ddd8322c720f4d1d30c44b724b.png

    PV = nRT

    3. The attempt at a solution

    [tex]\frac{\partial S}{\partial V}= \frac{nR}{V}[/tex]
    [tex]\frac{\partial S}{\partial P} = -\frac{nR}{P}[/tex]

    I found out S by doing the standard procedure: integrating the first one and deriving in relation to P to find the function in relation to P. The expression for S i found was:

    [tex]S=nR(lnV-lnP)[/tex]

    But the variation of S is always 0 this way, and that's not the solution...
     
  2. jcsd
  3. Jan 27, 2012 #2
    Did you get it yet? Think about what has to happen to double your volume yet double your pressure. Ordinarily when you double your volume what would you expect to happen to the pressure? And if you double the pressure, what would you expect to happen to the volume? So for these to happen together something else has to happen also.

    What do both of these changes do to the entropy of the system?
     
    Last edited: Jan 27, 2012
  4. Jan 28, 2012 #3
    No, I didn't find it yet. When the pressure and volume both double up, the temperature has to rise by 4x?
     
  5. Jan 28, 2012 #4
    Exactly. So intuitively you have to add heat to make system do this. Entropy rises with both an increase in volume and an increase in pressure. All the relations I've found though use specific heat. There are so many things you can calculate but I'm looking for something cut and dried relating entropy to both increase in volume and pressure although you can calculate the relative increase in temperature as you did and try to go from there. So I'm continuing to look and hoping someone who's more current on thermo for ideal gases will see this. another problem I'm running into is that I took physical chemistry (a year course) as a substitute for thermo (a semester course not nearly as rigorous) so there is a bit of a notation difference also. I'll keep trying and get back to you.
     
  6. Jan 29, 2012 #5
    Do you know the correct answer to this question?
     
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