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by philosopher-saint on November 22nd, 2009
Equivalent to your last forkfull of beans?!
;-)
by Glenn Blaylock on November 22nd, 2009
This sounds like a homework question. So, I am not going to tell you the answer. I will tell you how to get it.
First, you need to start with the universal gas law, PV=nRT. When starting with a constant amount of gas particles (n) and simply changing the pressure (P), volume (V), and/or temperature (T), then this equation can be rearranged thus PV/T=nR. When only those three values change, then PV/T for the beginning situation must equal PV/T for the ending situation. Thus, P1V1/T1 = P2V2/T2 where
P1 = starting pressure
V1 = starting volume
T1 = starting temperature
P2 = ending pressure
V2 = ending volume
T2 = ending temperature
With this equation, you can solve your problem. All you have to do is choose any starting values you desire and manipulate them according to the instructions. So, that would be temperature remains constant (T1 = T2), final volume is one half of the starting volume. So, pick a couple of sets of values for the variables run these through the equation and see what the relationship is between the change in volume and the change in pressure.
by BoobDaddy69 on November 22nd, 2009
Huh?
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You're reading A quantity of an ideal gas initially at atmospheric pressure is maintained at a constant temperature while it is compressed to half its volume. What is the final pressure of the gas?
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