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I tried reading some old threads, but keep getting confused. Can someone help make this more concise and tell me if this is right:
Ideal gas law assumptions include:
no volume
no IM forces
elastic (Kinetic energy and momentum conserved)
low Pressure
high Temperature
Deviations from ideal gas law:
high pressure
low Temperature
if Temperature decreases:
-IM becomes significant so less Pressure than expected
-smaller volume than predicted
if significantly increase pressure:
-larger volume because size becomes large compared to distance between them
if moderately increase pressure:
-volume less than predicted (why?? I read this in Kaplan and don't understand why V would be less with moderate increases but high with significant pressure increases)
if increase volume:
IM forces increases, so less pressure than expected
if decrease volume:
IM forces increases to higher pressure than expected
I feel like I'm confusing some concepts. Can anyone help? Thanks!!!!!!
Ideal gas law assumptions include:
no volume
no IM forces
elastic (Kinetic energy and momentum conserved)
low Pressure
high Temperature
Deviations from ideal gas law:
high pressure
low Temperature
if Temperature decreases:
-IM becomes significant so less Pressure than expected
-smaller volume than predicted
if significantly increase pressure:
-larger volume because size becomes large compared to distance between them
if moderately increase pressure:
-volume less than predicted (why?? I read this in Kaplan and don't understand why V would be less with moderate increases but high with significant pressure increases)
if increase volume:
IM forces increases, so less pressure than expected
if decrease volume:
IM forces increases to higher pressure than expected
I feel like I'm confusing some concepts. Can anyone help? Thanks!!!!!!