|Feb2-11, 12:07 PM||#1|
Gibbs Free Energy
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
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?
Or do I use a different equal for that? The volume of the box doesn't change, so would I use ?
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