1. The Ideal Gas Law and Kinetic Theory
Chapter 14

2. 14.1 Molecular Mass, The Mole, and Avogadro’s Number
Atomic mass unit: unit used to set up reference scale for masses as small as atoms
1 u = x kg
Based on experiment with Carbon-12, one mole of an element contains x 1023 atoms of that element. You should already be familiar with Avogadro’s Number.
The mass per mole of a substance has the same numerical value as the atomic or molecular mass
Using the periodic table, you should be able to convert between mass, moles, and particle numbers

3. 14.2 The ideal Gas Law
An ideal gas is a model for real gases that have particles so far apart that they do not interact
R is a proportionality constant called the universal gas constant. Experimentally determined, its value is 8.31 J/(mol K)

4. More ideal Gas law
Sometimes we express the ideal gas law in terms of the number of particles (N)instead of the number of moles(n).
In that case, use Boltzmann’s constant instead of the universal gas constant.
k = 1.38 x J/K
Remember: STP equals 273K and 1atm (101.3 kPa)

5. Review of Gas Laws Boyle’s Law Constant Temperature Charles’ Law
Constant Pressure
Gay-Lussac Law
Constant Volume
Use degrees Kelvin!

6. 14.3 Kinetic Theory of Gases
Any object in motion will have kinetic energy.
This statement is true for particles of a gas.
As a gas absorbs energy, the average kinetic energy of the particles will increase.
As a result, the temperature of the gas will increase.

7. Internal energy of monatomic ideal Gas
Internal energy is the sum of the various kinds of energy that the atoms or molecules of the substance possess.
For monatomic gases, the internal energy depends on the number of moles and the Kelvin temperature of the gas.
This relationship is true for any type of ideal gas.

8. 14.4 Diffusion
Diffusion is the process in which molecules move from a region of higher concentration to one of lower concentration.
Process is very similar (in concept and equation) to process of heat conduction.
Fick’s Law of Diffusion establishes a mathematical formula for explaining the mass of diffused solute in a given time
m is mass
D is diffusion constant
A is cross sectional area
C is concentration
t is time
L is length of channel