1. The Ideal Gas Law Objectives:
7.0 Explain the behavior of ideal gases in terms of pressure, volume, temperature, and number of particles using Charles's law, Boyle's law, Gay-Lussac's law, the combined gas law, and the ideal gas law.
6.0 Solve stoichiometric problems involving relationships among the number of particles, moles, and masses of reactants and products in a chemical reaction.

2. Intro
What will happen to the pressure in a tire as air is added, if the volume and temperature of the tire do not change?
So the amount of gas (moles) and the pressure both change.
Remember:
Combined Gas Law: P1V1 = P2V2
T T2

3. Ideal Gas Law
Since the ratio remains the same, then we can say it is constant. We call the constant k.
k is a constant based on the amount of gas (n) present, where k = nR. (R is an experimentally determined constant, called the ideal gas constant, and equal to L-atm/mol-K.
Ideal gas law equation: PV=nRT

4. What is an Ideal Gas? A gas that follows all the gas laws
When do gases not follow the gas laws?:
Gases tend not to behave “ideally” under very high pressures and low temperatures, as there is more inter-particular interactions.
Also, polar particles (like water vapor) are more attracted to each other because of their partial charges.
Large particles interact more.

5. Applying the Ideal Gas Law
PV=nRT:
What is n?
How can n be used to find the mass of a gas present?
From stoichiometry, what else can be determined from n? How??????
Substitutions in the ideal gas equation:
n = mass (m)/molar mass (M)
Rearrange the formula to solve for M.
Density (D) = ?????

6. Examples & Assignment Examples: p.437 (41, 45) and p.438 (46, 50)
Other Practice Problems can be used to practice and make sure you know how to solve problems.
Assignment:
Section Assessment: p. 439 (53, 55)
449: