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# chemnotes - Boyles Law Pressure vs Volume Pressure goes up...

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Boyle’s Law Pressure vs. Volume Pressure goes up, volume goes down Inverse relationship Pressure is inversely proportional to volume (Temperature and moles of gas are constant) P = 1/V If you double pressure you have to half volume PV = K (depends on n and T) P1V1=P2V2 for before and after scenario Any units will work Charles Law (hot air balloonist) Concerned with how volume related to temperature Knew if you heated a gas, the hotter you get it the more it would expand Volume related to temperature Volume is directly proportional to temperature Normally when you keep cooling a gas, you can get it smaller and smaller, but it turns into a liquid…. Volume drops to about a 1000 th of what it was…. Where you keep cooling a gas until it’s gone…which is impossible, it is an extrapolation which equals -273.15 degrees C = 0 degrees K and that is absolute zero Once you’re on the absolute scale, now your temp/volume is directly proportional but it HAS to be KELVIN!!! V/T = K - depends on pressure and number of moles (never changes) Avogadro’s Law Hold pressure and Temperature constant Moles = mass/molecular weight V1/n1=v2/n2 V ( any unit) n (have to be in moles)

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## This note was uploaded on 10/28/2009 for the course CH 53130 taught by Professor Mccord during the Fall '09 term at University of Texas.

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chemnotes - Boyles Law Pressure vs Volume Pressure goes up...

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