Gibbs Free Energy

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

    You have two parts of a tank, divided by a divider. On the larger side, you have 4 mol of N2 gas and on the smaller side you have 1 mol O2 gas. Both gasses are are the same T and P. The divider is removed and the gasses mix.

    What is the final T and P?

    What is the change in Gibbs Free Energy


    2. Relevant equations

    Daltons Law of Partial Pressure
    [​IMG]
    [​IMG]

    because T is constant

    3. The attempt at a solution

    So the final Temperature is the same as Ti because there is no chemical reaction

    The final Pressure is the sum of the Pressures of Po + Pn = Pf
    To solve this I just need Pf=2P ? (since each gas was at P pressure initially)

    For the Gibbs free energy, the entropy changes, as well as pressure. But how do I solve this?

    For the [​IMG]

    Or do I use a different equal for that? The volume of the box doesn't change, so would I use [​IMG]?
     
  2. jcsd
Know someone interested in this topic? Share a link to this question via email, Google+, Twitter, or Facebook

Have something to add?

0
Draft saved Draft deleted