1. Characteristics of Gases and KMT
Chapter 10

2. Characteristics of Gases
Unlike liquids and solids, they
Expand to fill their containers.
No definite shape or volume
Are highly compressible.
Have extremely low densities.
The effects of the attractive forces between the gases is minimal
Assume the molecules are moving independent of each other 2

3. Pressure F P = A Pressure is the amount of force applied to an area.
Atmospheric pressure is the weight of air per unit of area. 3

4. Units of Pressure Pascals 1 Pa = 1 N/m2 mm Hg or torr
These units are literally the difference in the heights measured in mm (h) of two connected columns of mercury.
Atmosphere
1.00 atm = 760 torr or 760 mm Hg 4

5. STP (Standard Temperature & Pressure)
Normal atmospheric pressure at sea level.
It is equal to
1.00 atm
760 torr (760 mm Hg)
kPa
Standard Temperature
0°C = 273 K 5

6. Kinetic-Molecular Theory
This is a model that aids in our understanding of what happens to gas particles as environmental conditions change. 6

7. Main Tenets of Kinetic-Molecular Theory
Gases consist of large numbers of molecules that are in continuous, random motion. 7

8. Main Tenets of Kinetic-Molecular Theory
The combined volume of all the molecules of the gas is negligible relative to the total volume in which the gas is contained.
Attractive and repulsive forces between gas molecules are negligible. 8

9. Main Tenets of Kinetic-Molecular Theory
Energy can be transferred between molecules during collisions, but the average kinetic energy of the molecules does not change with time, as long as the temperature of the gas remains constant.
Some molecules gain energy while others lose it
Conservation of energy within the system 9

10. Main Tenets of Kinetic-Molecular Theory
The average kinetic energy of the molecules is proportional to the absolute temperature. 10

11. Real Gases
In the real world (gases we typically are in contact with in the most lab settings), the behavior of gases only conforms to the ideal-gas equation at relatively high temperature and low pressure. 11

12. Deviations from Ideal Behavior
The assumptions made in the kinetic-molecular model break down at high pressure and/or low temperature.
Real gases deviate from ideal behavior:
At extremely high pressures (compresses molecule into liquid) that are not typically seen in lab
When intermolecular attractions occur between gas molecules
Distance dependent (only occur when molecules are close)
Example: during collisions
At sufficiently low temperatures (molecules condense into a liquid) 12