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Unknown (to me) formula of Entropy

  1. Apr 20, 2015 #1
    1. The problem statement, all variables and given/known data
    The question is says:
    Two vessels divided by a partition contain 1 mol of N2 and 2 mol of O2 gas. If the partition is removed and gases ate mixed isothermally, then find the change in entropy due to mixing assuming initial and final pressure are same .

    2. Relevant equations
    ΔS=qrev/T [the one I know]
    ΔSsys=-RΣniln xi
    Where ni = number of moles of gas.
    xi= mole fraction of gas.[ the foreigner equation]

    3. The attempt at a solution
    As written here in the relevant equations part, the second equation is the one which is new to me. I don't know how it works, what it does and from where it came from. It looks like boltzmann's entropy formula but I don't think that both of them are same. The question can be easily solved by this equation, but this equation is the one creating problem.
  2. jcsd
  3. Apr 20, 2015 #2
    What is R?
  4. Apr 20, 2015 #3
    Also, this at least looks related to the formula for change in entropy of an ideal gas.

    That is, taking the entropy of each which I believe, in general, is ##S= Nk[\log(Ω)]## where Ω is multiplicity. So taking the difference of two entropies gives you a ration of multiplicities inside the log. I don't know what formulas you have for multiplicity, but it seems like this may be where your equation comes from. Though, someone else can likely explain it better, or correct me.
  5. Apr 20, 2015 #4
    R is the universal gas constant.
    What is N here?
  6. Apr 21, 2015 #5
    Number of atoms.
  7. Apr 22, 2015 #6
    Smith and van Ness, Introduction to Chemical Engineering Thermodynamics, page 300:

    A ideal gas is a model gas comprised of imaginary molecules of zero volume that do not interact. Each chemical species in an ideal gas mixture therefore has its own private properties, uninfluenced by the presence of other species. This is the basis of Gibb's theorem:

    A total thermodynamic property (U, H, S, A, G) of an ideal gas mixture is the sum of the total properties of the individual species, each evaluated at the mixture temperature but at is own partial pressure.

  8. Apr 22, 2015 #7
    ΔSsys=-RΣniln xi
    Where ni = number of moles of gas.
    xi= mole fraction of gas.

    What would be the proof for this?
    Is it a complicated one involving partial derivatives?
  9. Apr 22, 2015 #8
    No. From the information I gave in my previous post, you should be able to derive the equation for the entropy change for mixing ideal gases, going from the pure components at pressure P to the mixture at the same pressure P.

  10. Apr 22, 2015 #9
    So S = V + P + T ?
    ΔS= ΔV + ΔP + ΔT ?
  11. Apr 22, 2015 #10
    Do you know how to determine the change in entropy of a pure species ideal gas if its pressure changes at constant temperature?
  12. Apr 22, 2015 #11
    Actually entropy is to me degree of randomness and also have formula,
    ΔS = Δq/T
  13. Apr 22, 2015 #12
    OK. Before you can do the derivation of the ideal gas entropy of mixing, you need to develop some background understanding of entropy. Did I send you my write up on the first and second laws of thermo?

  14. Apr 22, 2015 #13
    No, you till now have not send it. Why that question?
    I think you may be thinking that we had a discussion in some other thread about it?
    Or are you asking can I send you the write - up?
  15. Apr 22, 2015 #14
    No. I'll send you a link to it. It is for students who are struggling with some of the concepts because the concepts are presented so poorly in text books.
    Last edited: Apr 23, 2015
  16. Apr 22, 2015 #15
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