2. 1. Identify the four factors that affect gases. Pressure Volume Number of moles Temperature a. b. c. d. P V n T (Kelvin)

3. Dalton’s Law of Partial Pressures For a mixture of gases in a container, P Total = P 1 + P 2 + P 3 +... What is the total pressure on a container of nitrogen gas with a pressure of 10 kPa with oxygen gas with a pressure of 20 kPa and carbon dioxide with a pressure of 30 kPa? P total = 10 kPa + 20 kPa + 30 kPa P 1 = 10 kPa N 2 P 2 = 20 kPa O 2 P 3 = 30 kPa CO 2 P T = _____ kPa P total = P 1 + P 2 + P 3 P total = 60 kPa

4. A 1.0 L rigid cylinder contains 3 different gases (helium, nitrogen, and carbon dioxide). If the cylinder, helium gas has a pressure of 125 kPa, nitrogen has a pressure of 75 kPa and carbon dioxide has a pressure of 115 kPa. What is the total pressure of the gases exerted on the cylinder? P = PTPT = 312 kPa P = He 112 kPa 75 kPa = 125 kPa P = P T = 125 kPa+ 75 kPa+ 112 kPa PT =PT = ____ kPa N2N2 CO 2 P + He P + N2N2 P CO 2 PTPT (Example) Copy this work on your notes sheet.

5. Graham’s Law of Effusion or

6. Effusion Effusion: describes the passage of gas into an evacuated chamber.

7. Diffusion: describes the mixing of gases. The rate of diffusion is the rate of gas mixing. Diffusion

8. Two gases CH 4 and Cl 2 are released at the same time from opposite ends of the room. You are in the center of the room. Which gas will reach you first? (hint: mass of Cl=35.45; C=12.01; and H=1.01) Part A: Calculate the molar mass of each gas below Circle one: Methane (CH 4 )or Chlorine (Cl 2 ) Part B:How much quicker will the gas reach you? v 1 = CH 4 is 2.1 times faster than Cl 2 m 1 = m 2 = Lighter gases travel faster Cl 2 16.05 g/mol CH 4 v 2 = CH 4 16.05 70.90 Cl 2 = 70.90 g/mol 1.01 x 4 4.04 = 16.05 12.01 x 1 12.01 + 35.45 X 2 70.90 or =2.1 (Example) Copy this work on your notes sheet.

10. Kinetic Energy of Gas Particles At the same conditions of temperature, all gases have the same average kinetic energy. m = mass v = velocity

11. KE = ½ mv 2 A B Both objects at the same temperature. Same temp. means same KE ave KE A = KE B ½ m A v A 2 = ½ m B v B 2 multiply both sides by 2 22 m A v A 2 = m B v B 2 divide both sides by m A and V B 2 mAvB2mAvB2 mAvB2mAvB2 v A 2 m B mAmA vB2vB2 = Take the square root of both sides.

12. Graham’s Law of Effusion or