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Old Sep 28th 2011, 09:02 PM   #1
HelpmePLEASE
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Partial Pressures question

I'm not 100% sure how to solve this I tried using grahams law pv=nrt and even daltons partial pressure but I just cant so here it is:

Two chambers are connected by a valve. One chamber has a volume of 15.0 L and contains N2 gas at a pressure of 2.00 atm. The other has a volume of 1.50 L and contains O2 gas at a pressure of 3.00 atm. The valve is opened and the gases mix what is the final pressure in the system in atm?

I'm 100% sure it must regard effusion but I just don't know how
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Old Sep 28th 2011, 11:19 PM   #2
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Grahams Law, I would think is enough to solve this.

Assuming that T is constant, the total number of moles n is given by PV/RT. So,

P1V1/RT + P2V2/RT = PtVt/RT

Which gives:

P1V1 + P2V2 = PtVt

You have P1, V1, P2, V2 and Vt is adding V1 and V2. Can you solve for Pt?

t is total by the way.
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Old Oct 4th 2011, 05:39 PM   #3
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ya I got it thanks man!
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Old Oct 4th 2011, 10:36 PM   #4
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You're welcome!
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