1. Do Now 1/20/15 1. What is the combined gas law equation? 2. You have 17 L of gaseous F 2 at a pressure of 2.3 atm and a temperature of 299K. If you raise the temperature to 350K and lower the pressure to 1.5 atm, what is the new volume of your F 2 ? 3. What is the molar mass of oxygen gas?

2. Today’s Game Plan Do Now10 minutes Dalton’s Partial Pressure10 minutes The Ideal Gas Law20 minutes Independent Practice10 minutes Exit Ticket10 minutes

3. By the end of today’s class period, I will be able to…  calculate the partial pressure and total pressure of a gas mixture using Dalton’s law of partial pressures  calculate moles, volume, temperature, or pressure of a gas using the Ideal Gas Law

4. Dalton’s Law of Partial Pressure  states that the pressure of a gas mixture is the sum of the partial pressures of each individual gas in the mixture

5. What is Partial Pressure?  The pressure that the gas would exert if it were alone in the container What pressure would just the ‘red’ gas exert if it were alone in the container?

6. Dalton’s Law of Partial Pressures P total = P 1 + P 2 + P 3 … Pressure of the ‘red’ gas plus pressure of the ‘blue’ gas

7. Quick Solve and Write…  A 1.0L sample of Helium gas at 25°C and 1.5atm, and a 1.0L sample of Argon gas at 25°C and 2.0atm are evacuated into the same 1.0L container at 25°C. What is the total pressure of gas in the new container? How does your answer relate to Dalton’s Law of Partial Pressure?

8. Quick Solve and Write…  A 1.0L sample of Helium gas at 25°C and 1.5atm, and a 1.0L sample of Argon gas at 25°C and 2.0atm are evacuated into the same 1.0L container at 25°C. What is the total pressure of gas in the new container? If the total pressure of the gas is increased to 10.0 atm, what is the new pressure of helium?

9. Dalton’s Law of Partial Pressures 0.0atm

10. Dalton’s Law of Partial Pressures 0.0atm

11. Dalton’s Law of Partial Pressures 0.0atm

12. Dalton’s Law of Partial Pressures 0.0atm

13. Dalton’s Law of Partial Pressures 0.0atm

14. Dalton’s Law of Partial Pressures 0.5atm 0.4atm

15. Dalton’s Law of Partial Pressures 0.7atm 0.8atm

16. Dalton’s Law of Partial Pressures 1.2atm 1.8atm

17. Dalton’s Law of Partial Pressures 1.4atm 1.9atm

18. Dalton’s Law of Partial Pressures 1.5atm 2.0atm

19. Dalton’s Law of Partial Pressures 1.5atm 2.0atm 0.0atm

20. Dalton’s Law of Partial Pressures 1.5atm 2.0atm 0.2atm

21. Dalton’s Law of Partial Pressures 1.5atm 2.0atm 0.8atm

22. Dalton’s Law of Partial Pressures 1.5atm 2.0atm 1.7atm

23. Dalton’s Law of Partial Pressures 0.0atm 3.5atm

24. A Step Further… A sample of neon and oxygen gas has been collected into a 2.00 L bottle. The bottle is at room temp. (22.5°C) and contains 12.2 grams of oxygen and 25.5 grams of neon. If the total pressure is 12.5 atm, what are the partial pressures of each gas? How is this problem more difficult than the last problem??

25. Today’s Game Plan Do Now10 minutes Dalton’s Partial Pressure10 minutes The Ideal Gas Law20 minutes Independent Practice10 minutes Exit Ticket10 minutes

26. What are qualities of an ideal significant other?

27. But in reality…

28. An ‘Ideal’ Gas  A gas that obeys the equation PV=nRT  A gas behaves ideally when it exists close to Standard Temperature and Pressure

29. What is Standard Temperature and Pressure??  STP is 0°C and 1.00atm  The volume of 1 mole of an ideal gas at STP= 22.4 L

30. Quick Write: 2 min  In your notes, answer the following question: What is an ‘ideal gas’? Under what conditions do real gases behave most ideally?

31. The Ideal Gas Law  Used for a gas, when 3 of the 4 measurements are known and you want to find the 4 th  1. Volume  2. Pressure  3. Temperature  4. Moles

32. The Ideal Gas Law

33. PV=nRT  Pressure must be in atmospheres (atm).  Volume must be in liters (L).  Moles (make sure to convert grams to moles)  R is the gas constant= 0.08206 Latm/molK  Temperature must be in Kelvin (K).

34. PV=nRT (Class Example) What volume is occupied by 0.250 mol carbon dioxide gas at 25°C and 371 torr?

35. PV=nRT (You Try)  What mass of neon gas (in grams) is required to fill a 5.00-L container to a pressure of 1.02 atm at 25°C?

36. Today’s Game Plan Do Now10 minutes Dalton’s Partial Pressure10 minutes The Ideal Gas Law20 minutes Independent Practice10 minutes Exit Ticket10 minutes

37. PV=nRT Independent Practice  Silently and Independently begin on your homework assignment

38. Today’s Game Plan Do Now10 minutes Dalton’s Partial Pressure10 minutes The Ideal Gas Law20 minutes Independent Practice10 minutes Exit Ticket10 minutes

39.  PV=nRT  R = 0.08206 Latm/molK