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•WE’RE IN THE HOME STRETCH!•FINAL EXAM ONE WEEK FROM TODAY @ 8AM
•MAKE UP LAB
•OWL ASSIGNMENT WILL BE POSTED WED., COMPLETE BY SATURDAYChapter 10: Gases (Mon. & Wed.)
Chapter 11: Intermolecular Forces and the Liquid State (Fri.)
December 7, 2009
Gases
Why gases?
What is a gas? State of matter where distance between particles is
much bigger than the particles
Properties of Gases
Property Common Unit Other UnitsSymbo
l
Mass grams (g) mg, kg -
Amount moles (mol) none n
Volume liters (L) mL V
Pressureatmosphere (atm)
bar, mmHg, psi, kPa
P
Temperature
Kelvin (K) ºC, ºF T
Properties of Gases: What is pressure?
Area
ForcePressure
Common Units of Gas Pressure
1 atm =
1.013 bar
101.3 kPa (kilopascal)
760 torr
760 mmHg (mm mercury)
14.7 psi (pounds per sq. inch)
Kinetic Molecular Theory (Sec. 10.6)
Molecules in a gas are always moving quickly and randomly
Average kinetic energy is determined by temperature
All gases at the same temperature have the same average kinetic energy, regardless of mass
Gas molecules collide with each other and the walls of their container without losing energy (“elastic” collisions)
Kinetic Energy of Gases
Kinetic energy of a single molecule
Average kinetic energy for a collection of molecules:
velocityvmassmwheremvKE ,2
1 2
molKatmL0.082057
KmolJ8.3145constantgas
,Kelvininetemperatur2
3
2
1 2
R
T
RTvmKE
How fast do molecules really move?
O2 gas at room temperature (25ºC = 298K)
Root-mean-square (rms) speed
molkginmassmolarMmolKJRM
RTvvrms /,/3415.8
32
Boltzmann Distribution
Gas molecules move with a range of speeds
On average, gas molecules move faster at higher temperatures
Heavier gases move more slowly on average than lighter gases at the same temperature
Don’t confuse average kinetic energy with speed!