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

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
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)
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}

Page1 / 4

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

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online