Download presentation
Presentation is loading. Please wait.
Published byHendri Sanjaya Modified over 6 years ago
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
Similar presentations
© 2025 SlidePlayer.com. Inc.
All rights reserved.