1. Quiz – Get out your notes!!

2. Quiz (10 questions) 1) Which law would you use if you were given only pressure and volume? 2) Which law would you use if you were given only temperature and volume? 3) Which law would you use if you were given pressure, temperature, and volume?

3. Quiz (10 questions) 4) If I increase the temperature in a sample of gas, what happens to the motion of the particles? 5) If the particles collide more frequently with the sides of the container, does the pressure increase or decrease?

4. Quiz (10 questions) 6) A sample of gas at 47°C and 1.03 atm occupies a volume of 2.20 L. What volume would this gas occupy at 107°C and 0.789 atm? 7) A sample of air has a volume of 140 mL at 67°C. At what temperature will its volume be 50 mL at constant pressure?

5. Quiz (10 questions) 8) Convert 15°C to Kelvin. 9) Convert 2.5 atm to mm Hg. 10) Convert 236505 Pa to torr.

6. Dalton’s Law of Partial Pressures

7. Dalton’s Law Proposed by John Dalton Proposed by John Dalton Says that the pressure of a gas mixture is the sum of the individual pressures of each gas present Says that the pressure of a gas mixture is the sum of the individual pressures of each gas present P T = P 1 + P 2 + P 3 +….. P T = P 1 + P 2 + P 3 +…..

8. Example A balloon contains a mixture of carbon dioxide, nitrogen, and oxygen. The total pressure of the balloon is 760 torr. The partial pressure of the carbon dioxide is 0.285 torr and the partial pressure of the nitrogen is 593.525 torr. What is the partial pressure of the oxygen? A balloon contains a mixture of carbon dioxide, nitrogen, and oxygen. The total pressure of the balloon is 760 torr. The partial pressure of the carbon dioxide is 0.285 torr and the partial pressure of the nitrogen is 593.525 torr. What is the partial pressure of the oxygen? 760 = 0.285 + 593.525 + P O2 760 = 0.285 + 593.525 + P O2 P O2 = 166.190 torr P O2 = 166.190 torr

9. Practice page 35 A container of gas contains nitrogen, oxygen, and helium. The pp of the oxygen is 0.235 atm, the pp of the nitrogen is 0.715 atm, and the pp of the helium is 0.050 atm. What is the total pressure of the gas? A container of gas contains nitrogen, oxygen, and helium. The pp of the oxygen is 0.235 atm, the pp of the nitrogen is 0.715 atm, and the pp of the helium is 0.050 atm. What is the total pressure of the gas?

10. Practice The total pressure of a contained sample of gas is 1.53 atm. The sample contains chlorine gas with a pp of 0.203 atm, neon gas with a pp of 0.830 atm, and an unknown gas. What is the pp of the unknown gas? The total pressure of a contained sample of gas is 1.53 atm. The sample contains chlorine gas with a pp of 0.203 atm, neon gas with a pp of 0.830 atm, and an unknown gas. What is the pp of the unknown gas?

11. Practice If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature?

12. Practice If I have an unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 liters, and a temperature of 87 K, how many moles of gas do I have? If I have an unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 liters, and a temperature of 87 K, how many moles of gas do I have?

13. Practice If I contain 3 moles of gas in a container with a volume of 60 liters and at a temperature of 400 K, what is the pressure inside the container? If I contain 3 moles of gas in a container with a volume of 60 liters and at a temperature of 400 K, what is the pressure inside the container?