1. PV= nRT KMT P= nRT – a(n/V)2 V-nb Gases Stoich. urms= (3RT/MM)1/2
Units
mm, torr, atm, Pa, kPa, N/cm2
A.P. Chem. Ch. 5
Gases
Pressure: Force Area
CaPtot= Pa
Dalton’s Law Ptot= Pa+ Pb…
Boyle’s Law PV=k
Charles’ Law V/T=k
Avog. Law V/n=k
Graham’s Law Ra/Rb = (MMb/MMa)1/2
Stoich.
Devices
Barometer
At STP
Manometer
L atm/mol K 8.31 J/ mol K
22.4 L = 1 mole
PV= nRT
The way we choose to view it
Non- STP
P = dRT/MM
Derivation
KMT
P = 2 nNA1/2mu2 3V
P = 2 nKE
urms= (3RT/MM)1/2
Dimensionless Pts.
The Way It Really Is. 3V
KEper mole = 3/2 RT
In constant motion
Colliding 100% elast.
Particle interactions
Creating pressure
P= nRT – a(n/V)2
w/o influence
In such a way that Temp is dir. Prop. To average KE.
V-nb
Volumes of particles