|Feb19-13, 03:53 PM||#1|
Basic Ideal Gas Law Question
Perhaps I have some mental block with basic algebra (so don't judge me on that), but...
Here is a simple high-school level question regarding ideal gas laws:
If I have two fixed chambers "a" and "b", both of equal volume connected in the middle with a compressor, and I compress gas taken from "a" and move it to "b", does the temperature in "b" rise, while the temperature in "a" falls (excluding heat exchange with the environment)?
i.e. the volumes remain constant, but the pressure in "b" rises. The pressure in "a" falls. Does the temperature do anything?...during compression, some of the moles of gas will move from a to b as well...correct?
I hope you understand where I'm confused.
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|Feb19-13, 03:59 PM||#2|
To compress the gas you do some work on it, so it is not a simple application of the ideal gas equation.
|Feb19-13, 04:06 PM||#3|
Which equation would one use?
To be more specific, I'm trying to figure out how much work.
Both chambers are equal volume.
Gas = Nitrogen (or some ideal gas)
They both start out at P0 = 2 atm pressure.
They both start out at T0 = 300K
From there, we compress from "a" to "b", until chamber "b" is at 3 atm, and chamber "a" is at 1 atm.
How much work, and how does that affect the temperature in "a" and "b"?
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