BENG 130 Lecture 2: Lecture 02
Document Summary
Boyle"s experiments with pressure, volume, and temperature: saw that p*v is proportional to t, thus, we got (cid:1842)(cid:1848)=(cid:1866)(cid:1844) This is the ideal gas law: assumptions of ideal gas law. 2) no interatomic/molecular forces: if we have multiple i gases: Van der waals" modifications to account for non-ideal gases: first, he took care of assumption 1 (point masses), next, he took care of assumption 2 by subtracting the pull of the gases: (cid:1842)= normally, but now (cid:1842)= (cid:3029) to account for non-point masses. A and b are constants that depend on the gas. (cid:1831)= (cid:1856)(cid:1831)=0: energy is a state function . In other words, energy only depends on the state! It does not depend on the path: let"s say we have a gas that we take from state 1 to state 4. (cid:1831)=(cid:2869)(cid:2870)(cid:1865)(cid:1731)(cid:2872)(cid:1732)(cid:2870) (cid:2869)(cid:2870)(cid:1865)(cid:1731)(cid:2869)(cid:1732)(cid:2870)=(cid:2869)(cid:2870)(cid:1865)[(cid:1731)(cid:2872)(cid:1732)(cid:2870) (cid:1731)(cid:2869)(cid:1732)(cid:2870): if we went from 1 to 2 to 3 to 4:
