1. Kinetic Molecular Theory of Gases

2.  Kinetic Molecular Theory of Gases- is a model that attempts to explain the properties of an ideal gas.  An ideal gas is a gas in which the particles are considered to have no mass and these particles exert not attraction for each other.  Real Gas - real gas particles have volume and feel an attraction for each other. At low pressures and/or high temperatures, real gases generally behave ideally.

3. Kinetic Molecular Theory  1. Ideal gas particles are separated by vastly large spaces in comparison to the particle size.  2. Ideal gas particles move in a completely random motion and build pressure by colliding with their container and each other.  3. Ideal gas particles have no attraction for other ideal gas particles.  4. The average kinetic energy (motion of particles) is directly proportionate to the average temperature of the particles.

4. Standard Temperature and Pressure  The Kinetic Molecular Theory mentions a gas has a force called pressure from colliding with itself and the walls of its container. Pressure = force/area.  It also states the motion of the particles that cause pressure is related to temperature. More kinetic energy (motion) means a higher temperature.  Since pressure and temperature can vary, standard values are set in order to compare gases.

5.  Standard Temperature Values  0 o C or 273 o K  The Kelvin scale will never go below 0K, absolute zero.  o C = o K - 273  o K = o C + 273  How many O K are in 400 o C?  o K = o C + 273  o K = 400 o + 273  o K = 673  Standard Pressure Values  1 atm  101.3 kPa  760 mm Hg or 760 torr  How many atm are in 300.kPa?  300kPa * 1atm = atm 101.3kPa  atm = 2.96

6. KMT Questions  A gas can be described by 3 factors: pressure, volume, and temperature. We will talk about numerous formulas that will relate these factors.  What happens to pressure if you increase the temperature of a gas?  What happens to temperature if you decrease the volume in a container?  What happens to the volume of a flexible container if the pressure is increased?

7. Effusion -is a process by which gas particles pass through a small opening. The rate of effusion of different gases is directly proportional to the velocity of their particles and their mass.

8. Diffusion- is spontaneous mixing of the particles of two substances caused by their random motion.