1. IDEAL GAS LAW PV=nRT

2. IDEAL GAS LAW P=pressure (in kPa or atm only!) V= volume in Liters n = number of moles R= Ideal Gas Law Constant T= Temperature in KELVIN

3. IDEAL GAS LAW R= 8.31 kPa*L Mole*K Or R=.0821 atm*L mole * k **Units must cancel in what you plug into the equation!!!

4. IDEAL GAS LAW Ideal gases are those that are: Not affected by intermolecular forces Behave according to the Kinetic molecular theory

5. IDEAL GAS LAW Avagadro’s Principle: Equal volumes of gases at the same temperature and pressure contain the same numbers of particles 1 mole= 22.4 L of gas= 6.023 x 10 23 atoms/molecules

6. IDEAL GAS LAW In reality, no gas is ideal. Under the right conditions, calculations with the ideal gas law will be very close to real gases.

7. IDEAL GAS LAW GRAPH Shows how accurately the ideal gas law can be used to estimate the characteristics of a real gas.

8. IDEAL GAS LAW GRAPH

9. The closer the real gas is to the ideal gas line (constant), the better the estimation will be.

10. IDEAL GAS LAW GRAPH

11. Examples 1. 3.25 g of XeF4 gas is placed into an evacuated 5.00 liter container at 80.0 °C. What is the pressure in the container?

12. Examples 2. What is the temperature if 1 mole of O 2 occupying 100 L of volume has a pressure of 20 Pa (1000 Pa=1 KPa)?

13. Examples 3. A 334 mL cylinder for use in chemistry lectures contains 8.470 g of helium at 23oC. How many grams of helium must be release to reduce the pressure to 145 atm assuming ideal gas behavior? (Atomic weight: He = 4.00).