[neact] Re: Gas law related question
- From: Peter Nassiff <pnassiff@xxxxxxxxx>
- To: neact@xxxxxxxxxxxxx
- Date: Thu, 23 Jul 2009 07:55:55 -0700 (PDT)
Look up the clausius-clapeyron equation. You can find it in Chemistry, Central
Science or on the web.
--- On Wed, 7/22/09, Jerusha Vogel <jj@xxxxxxxx> wrote:
From: Jerusha Vogel <jj@xxxxxxxx>
Subject: [neact] Gas law related question
To: neact@xxxxxxxxxxxxx
Date: Wednesday, July 22, 2009, 9:28 PM
I have an interesting question that was posed to me and I
would appreciate some help in figuring it out.
imagine one has a container with a fixed volume (say 1L )
that has been filled with ½ L of water and hermetically sealed at room
temperature
and standard pressure (1atm). then the container is uniformly and slowly
heated. Is there a calculation that could be done to plot the change in
pressure of the gas above the water with increasing temperature up to say 100
deg C? is the pressure/temperature graph of the gas the same as that of the
liquid (considering one is compressible and the other is not)? is the graph
linear throughout? maybe it is horizontal? what happens after 100C (lets say to
120 degrees C)? is there a point where the water is completely evaporated (is
PV=nRT applicable at this point)?
Obviously we need to figure how the temperature increase
will affect the speed of the gas molecules, how many more gas molecules will be
produced as the water vaporizes, and then how equilibrium will force the
reaction backwards (due to the increased pressure) slowing down how the
molecules being released. PV=nRT might work moderately well at the start,
but as we get higher and higher pressure it becomes less useful and since there
would be different gases (n) involved, I’m not sure what to use for the
van der walls modification.
Do you think there is any way to calculate this or would it
have to be done by experiment only?
Any insight/suggestions on how to solve this problem would
be much appreciated.
Thanks,
Jerusha Vogel
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