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Can someone explain this to me please..

answer is C, because at extremely high pressures, the volumes of molecules come in to play.Can someone explain this to me please..
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Can someone explain this to me please..
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Can someone explain this to me please..
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It is assumed that ideal gases are point particles. A deviation in ideal behavior where molecular volume dominates would give a PV/RT of greater than one for one mole of methane.
I suck at gas law stuff. However, if I remember correctly, at Ideal conditions, pressure is low and temperature is high. Using that principle, "A" seems like a reasonable answer. Can anyone tell me if I'm right or wrong on this one?
Deviation to Ideal conditions = High Pressure, Low Temp...which would amount to a greater ratio than at ideal
Yeah, but the question isn't about an ideal gas, it's asking how methane acts in relation to an ideal gas
I actually think the answer is C, because high pressure means smaller container volume, which means the size of the molecules become important (ideal behavior is LOW pressure)
EDIT: I actually found something that illustrates exactly that: http://library.thinkquest.org/C006669/media/Chem/img/PV.gif
prsndwg, is there an answer key?