CHM 113 Lecture Notes - Lecture 1: Van Der Waals Equation, Van Der Waals Force, Ideal Gas Law
Document Summary
A gas can be described by 4 variables: p,v,t,&n. Force per unit area exerted on a surface (ex: container walls) Units: atm, mmhg (torr), pa, barr, psi. 1 atm = 1. 01325 x 10 5 pa = 101. 325 kpa. 1 bar = 10 5 pa = 0. 9869 atm. How hot or cold, and a measure of average velocity and kinetic energy of gas particles. At stp, 1 mole of an ideal gas occupies 22. 41 l. 1 mole = 6. 022 x 10 23 gas particles. Gas particles: can be atoms (he, kr, ar) or molecules (o 2 , ch 6 ) A real (actual) gas can"t be explained with simple equations. For an ideal gas, the 3 gas laws combine to glue: pv=nrt. Uses p,v,t or n when 3 variable are known. Determine the mass/molar mass of a gas sample: assm. These assumptions are more reasonable at low p and high t.
