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Heyy, I posted this before but it kinda got pushed down and ignored, and I was hoping maybe DrBob might have an idea since no one else did! okay I have this question about chemistry and its driving me nuts. It feels like I am so close but am just missing something. The question is:

A vessel of 6.84 L in volume contains 3.61 L of pure water at 25°C. A partial pressure of 3.67 atm of CO2 is quickly injected into the space above the water. Calculate the partial pressure of carbon dioxide remaining once the solution has become saturated with the gas. Henry's constant for CO2 at this temperature is 0.0350 M atm-1

Okay so I know basically this...we dicussed with some other people and rearrganed equations and basically got this:
(mol initial - mol final)/V = concentration x pressure.

so the initial moles you get using PV=NRT, so N=PV/RT and same for moles final (diff volumes used of course) but I think that's where I'm messing up. Because after that you divide by a volume, then by the concentration. But I think I'm messing up what volumes go where. I know what the answer ius supposed to be and I cant get it for the life of me. I'm thinking that for inital moles the volume would be 6.84 cause that's the whole thing. And then I'm thinking for final moles it would be 3.61 cause that's where the liquid is. But I don't know what I would divde by...the leftover 3.23? anyways I've tried many combinations and I cant get it. ANy help would be greatly apprecaited. I could be totally on the wrong track. Thanks

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Thanks.

=)

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