1. Behavior of Gases

2. Learning Goals Explain the Kinetic Molecular Theory
Describe the behavior of gases
Define gas pressure

3. Kinetic-Molecular Theory
Kinetic-molecular theory explains the different properties of solids, liquids, and gases.
The kinetic-molecular theory describes the behavior of matter in terms of particles in motion.

4. Kinetic-Molecular Theory
Gases are composed of separate, tiny (invisible) particles (atoms or molecules). The particles of a gas are extremely far apart.
Under ordinary conditions gases consist mainly of empty space.

5. Kinetic-Molecular Theory
Gas particles are in constant, random, linear, motion.
Gas particles travel in straight lines.
The direction that gas particles travel is random.

6. Kinetic-Molecular Theory
The kinetic energy of gas particles is directly proportional to their Kelvin temperatures.
The gas particles move faster as the temperature increases.
Temperature is a measure of the average kinetic energy of the gas particles.
Individual gas particles have different kinetic energies.

7. Kinetic-Molecular Theory
Collisions between gas particles or between gas particles and their container are elastic.
There is no energy transfer when gas particles collide.

8. Kinetic-Molecular Theory
The particles of a gas are not attracted or repelled by one another.

9. Behavior of Gases
Gases easily flow past each other because there are no significant forces of attraction.
Diffusion is the movement of one material through another.
Effusion is a gas escaping through a tiny opening.

10. Gas Pressure Pressure is defined as force per unit area P = force/area
Gas particles exert pressure when they collide with the walls of their container.

11. Gas Pressure
The particles in the earth’s atmosphere exert pressure in all directions called atmospheric air pressure.
There is less air pressure at high altitudes because there are fewer particles present, since the force of gravity is less.

12. Gas Pressure
Barometers are instruments used to measure atmospheric air pressure.

13. Gas Pressure
Manometers measure gas pressure in a closed container.

14. Gas Pressure The SI unit of force is the newton (N).
One pascal(Pa) is equal to a force of one Newton per square meter or N/m2.
One atmosphere is equal to 760 mm Hg or kilopascals.

16. Gas Pressure
Dalton’s law of partial pressures states that the total pressure of a mixture of gases is equal to the sum of the pressures of all the gases of the mixture.

17. Gas Pressure
The partial pressure of a gas depends on the number of moles, size of the container, and temperature and is independent of the type of gas.
At a given temperature and pressure, the partial pressure of 1 mol of any gas is the same.

19. Gas Pressure Ptotal = P1 + P2 + P3 +...Pn
Partial pressure can be used to calculate the amount of gas produced in a chemical reaction