1. Essential Questions EQ: How do we use the Ideal Gas Law? HOT Q1: What is the Ideal Gas Law? HOT Q2: When do we use the ideal gas law vs. combined gas law? HOT Q2: What is the Law of Partial Pressures? Warm Up 1) What Gas Law have we learned about so far? 2)When I open the door to Ms. Shank’s room next door, the combined air pressure is 5 atm. The air pressure inside only my classroom was 3 atm. What was the pressure in Ms. William’s room?

2. Agenda Warm Up Intro: Ideal Gas Law Flash! Ideal vs. Combined Quiz Return Partial Pressures Exit Ticket

3. Reminder MONDAY IS THE UNIT 2 TEST!!! Here for tutoring/retakes after school today (last day for Unit 1 Retakes) Worksheet #3 is HW

4. Notes: Ideal Gas Law PV = nRT “piv nert” This equation is used to predict any of these variables when the others are held constant. P = pressure (atm) V = volume (L) n = number of particles (moles) T = temperature (KELVIN!) R = gas constant - 0.0821 L atm mole K

5. When Do I Use Which? Use “Ideal Gas Law” when solving for a variable and everything is held constant… used “Combined Gas Law” when something is changing and you are asked for “new” pressure, for example. Think C ombined … C hange

6. Example The temperature inside my refrigerator is about 4 0 Celsius. If I place a balloon in my fridge that initially has a temperature of 22 0 C and a volume of 0.5 liters, what will be the volume of the balloon when it is fully cooled by my refrigerator? Are you changing pressure, volume, temperature, or # of particles? Ideal or Combined?

7. Example If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 L, what is the temperature? Are you changing pressure, volume, temperature, or # of particles? Ideal or Combined?

8. Flash! 1.0 L of a gas at 1 atm is compressed to.473L. What is the new pressure of the gas? Are you changing pressure, volume, temperature, or # of particles? Ideal or Combined?

9. Flash!.89 moles of a colorless gas occupy a volume of 84.1 L and a pressure of 3.6 atm. What is the temperature of the gas? P = 3.6 atm V = 84.1 L n =.89 mol T = ?

10. Flash! Synthetic diamonds can be manufactured at pressures of 60,000 atm. If we took 2.0 liters of gas at 1.0 atm and compressed it to a pressure of 60,000 atm, what would the volume be? Are you changing pressure, volume, temperature, or # of particles? Ideal or Combined?

11. Flash! If I have 8 moles of a gas at a pressure of 1.6 atm and a volume of 6 L, what is the temperature? Are you changing pressure, volume, temperature, or # of particles? Ideal or Combined?

12. Flash! If I have an unknown quantity of gas held at a temperature of 1195 K in a container with a volume of 25 liters and a pressure of 560 atm, how many moles of gas do I have? Are you changing pressure, volume, temperature, or # of particles? Ideal or Combined?

13. Examples A gas under a pressure of 2.3 atm and at a temperature of 293 K occupies a 500.0 L container. How many moles of gas are in the container? 1)P = 2.3 atmV = 500.0 L n = ? T = 293 K R = gas constant - 0.0821 L atm Kmole

14. Example If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 L, what is the temperature?

15. Partner Practice.89 moles of a colorless gas occupy a volume of 84.1 L and a pressure of 3.6 atm. What is the temperature of the gas?

16. Partner Practice If I have an unknown quantity of gas held at a temperature of 1195 K in a container with a volume of 25 liters and a pressure of 560 atm, how many moles of gas do I have?

17. Partner Practice If I have 8 moles of a gas at a pressure of 1.6 atm and a volume of 6 L, what is the temperature?

18. Notes: Partial Pressure Dalton's Law of Partial Pressure = The pressure of a mixture of gases is equal to the sum of the pressures of all of the individual gases alone. Pressure Total = Pressure 1 + Pressure 2... Pressure n IT’S NOTES TIME!!!

19. Wait….what? Let’s do a little demo: I need 3 volunteers It’s that easy!

20. Example A container holds parts of oxygen, nitrogen, and helium gas. The total gas pressure is 30 atm. If oxygen takes holds 12 atm of pressure and nitrogen holds 11 atm, what pressure is given off by helium? I LOVE NOTES!!

21. Example 2 A container holds both carbon and oxygen gasses. If oxygen gives off 3 atm of pressure and carbon gives off 9 atm of pressure, what is the total pressure of the container? Pressure Total = Pressure 1 + Pressure 2... Pressure n Pressure total = 3 atm + 9 atm

22. You try! The total pressure in a container holding oxygen, nitrogen, and carbon gas is 22 atm. If both oxygen and nitrogen give off 7 atm of pressure, what pressure is given off by carbon??

23. You Try! The total pressure in a system is 45 atm. The container holds four gases, oxygen; helium; hydrogen; and carbon. If oxygen and helium each give 8 atm, and carbon gives 14 atm, how much pressure is given off by hydrogen?

24. You Try! When combined, two gases have a pressure of 4.0 atm. If one gas has a pressure of 1.5 atm, what is the pressure of the second gas?

25. Exit Ticket 1) 0.8 moles of an ideal gas are stored in a 5L container at 1.5atm. What is the Temperature of the gas? 2) The total pressure in a closed system containing N 2, O 2, and CO 2 is 30 atm. If the partial pressure of N 2 is 4 atm, and the partial pressure of O 2 is 6 atm, what is the partial pressure of CO 2 ? HOMEWORK: Worksheet #3