|
1
|
|
|
2
|
- Particles of matter are ALWAYS in motion
- Volume of individual particles is » zero.
- Collisions of particles with container walls cause pressure exerted by gas.
- Particles exert no forces on each other.
- Average kinetic energy µ Kelvin
temperature of a gas.
|
|
3
|
- Kelvin temperature is an index of the random motions of gas particles
(higher T means greater motion.)
|
|
4
|
|
|
5
|
|
|
6
|
|
|
7
|
|
|
8
|
- Is caused by the collisions of molecules with the walls of a container
- is equal to force/unit area
- SI units = Newton/meter2 = 1 Pascal (Pa)
- 1 standard atmosphere = 101.3 kPa
- 1 standard atmosphere = 1 atm =
|
|
9
|
|
|
10
|
- Gases expand to fill their containers
- Gases are fluid – they flow
- Gases have low density
- 1/1000 the density of the equivalent liquid or solid
- Gases are compressible
- Gases effuse and diffuse
|
|
11
|
- P = 1 atmosphere, 760 torr, 101.3 kPa
- T = 0°C, 273 Kelvins
- The molar volume of an ideal
gas is 22.42 liters at STP
|
|
12
|
|
|
13
|
|
|
14
|
|
|
15
|
- The volume of a gas is directly proportional to temperature, and
extrapolates to zero at zero Kelvin.
|
|
16
|
|
|
17
|
|
|
18
|
|
|
19
|
|
|
20
|
|
|
21
|
- PV = nRT
- P = pressure in atm
- V = volume in liters
- n = moles
- R = proportionality constant
- T = temperature in Kelvins
|
|
22
|
|
|
23
|
|
|
24
|
|
|
25
|
|
|
26
|
|
|
27
|
|
|
28
|
- For a mixture of gases in a container,
- PTotal = P1 + P2 + P3
+ . . .
|
|
29
|
|
|
30
|
- Effusion: describes the passage
of gas into an evacuated chamber.
|
|
31
|
|
Notes
