1. Gases

2. Properties of Gases
Fluid
Low density
Expand to fill container
Effuse/ Diffuse
Compressible
Exert pressure

3. Effusion- gas particles push through a tiny opening in a container
Diffusion- gas particles mix freely due to kinetic molecular theory (KMT)

4. Pressure Force on a surface Units of pressure
1atm=760.mmHg= kPa=760.torr=1.0bar=14.7psi=101325Pa
You can convert from one pressure unit to another using dimensional analysis

5. 1atm=760.mmHg=101.325kPa=760.torr=1.0bar=14.7psi=101325Pa
2.18atm =_______ psi
mmHg=______kPa
174.21kPa =_______atm

6. Kinetic-Molecular Theory
Assumptions
large number of particles very far apart relative to their size.
all collisions are elastic.
no loss of kinetic energy.
particles in constant, rapid, random motion
no IMF exist among particles
average kinetic energy depends solely on temperature

7. Ideal vs Real Gases Ideal gases obey all assumptions of KMT Real gases
imaginary
Nobel gases almost always act ideally
Real gases
at high pressure or low temperature
IMF exist
Not all of the assumptions apply