March 24, 2015

1. March 24, 2015

2. april14, 2015 • What are the two types of gas stoichiometry questions? • How many moles of H2O are present in 2.24 L at 23 degrees C at 92.5 kPa. R is 8.314 • How many grams of NaOH can be produced from the mols of H2O above 2Na + 2H2O  2NaOH + H2 4. How do you know which reactant is limiting? 5. What is the formula for percentage yield?

3. April 14, 2015 5. Partial Pressure 6. KMT 7. Review 8. Quiz on Friday

4. April 8, 2015 2. Gas Laws – review 3. Ideal Gas Law 4. Gas Stoichiometry

5. TOPICS • Properties of Gases • Gas Laws • Ideal Gas Law • Gas Stoichiometry • Partial Pressure • Kinetic Molecular Theory • Effusion & Diffusion • Real Gases

6. What happens to an open can of soda after you leave it out? Why? Which can would go “flat” quicker, a cold can of soda, or a warm can of soda?

7. 1. Properties of GASES OBJECTIVE: Properties of Gases

8. Review • Play file 75185 and 75187

9. 5.1 Properties of gases • Has mass • Has volume • Low density • Creates Pressure

10. 5.1 & 5.2 Properties of gases What is Pressure? We live at the bottom of an ocean of air each collision = PRESSURE

11. 5.1 & 5.2 Properties of gases UNITS for pressure 1 atm 760 torr 760 mm Hg 101.325 kPa What is Pressure? We live at the bottom of an ocean of air each collision = PRESSURE

12. 1. Properties of gases Summary & Review 1. List three properties of gases 2. What is pressure? 3. What are the two units of pressure we will use in this class?

13. 2 Gas laws OBJECTIVE: Properties of gases with numbers

14. 5.3 Gas laws Boyle’s Law Relationship between PRESSURE and VOLUME when Temperature is held constant. P1V1= P2V2

15. 5.3 Gas laws P1 = initial pressure P2 = pressure after V1 = initial volume V2 = volume after P1V1= P2V2

16. 5.3 Gas laws UNITS P = kPa, atm, Volume = mL or L

17. 5.3 Gas laws

19. 5.3 Gas laws Volume , pressure ________ Pressure , volume ________ Volume , pressure _________ Pressure , volume __________

20. Boyle’s law Practice Problem A 2.5 L balloon has a pressure of 110.0 kPa. You shrunk the balloon’s volume to 1.25 L. What is the new pressure? P1V1= P2V2 (110.0 kPa)(2.5 L) = P2(1.25 L) (110.0 kPa)(2.5 L) = P2 (1.25 L)

21. Boyle’s law Practice Problem A car airbag inflated to a volume of 4.55 L with a pressure of 5.5 atm. The original pressure was 0.5 atm. What was the original volume? P1V1= P2V2 (0.5 atm)V1 = (5.5 atm)(4.55 L) V1= (5.5 atm)(4.55 L) (0.5 atm)

22. What is temperature? “How hot or cold it is.” What does it mean for something to be hot?

23. HEAT • is a form of energy • is kinetic energy What does this mean? Heat = how fast atoms/molecules are vibrating/moving

24. 1. INTERMOLECULAR FORCES What if we could measure how fast the atom/molecules are vibrating/moving? We can! We call this “temperature”!

25. 1. INTERMOLECULAR FORCES Temperature • measures heat • measures average kinetic energy of particles

26. 1. INTERMOLECULAR FORCES A high temperature means atoms/molecules… And a low temperature means…

27. Boyle’s law Summary & Review • What is the difference between heat and temperature • What does Boyle’s law state about pressure and volume?

28. Charles’s law OBJECTIVE: VOLUME and TEMPERATURE

29. 5.3 gas laws CHARLES’S LAW Relationship between TEMPERATUREand VOLUME at constant PRESSURE

30. Charles’s Law V1 = Initial Volume V2 = Volume After T1 = Initial Temperature T2 = Temperature After

31. Charles’s Law UNITS Volume = cm3, mL L Temperature = K Celsius + 273 = K

32. Charles’s Law

33. 6. Charles’s law Volume , Temperature ________ Temperature , Volume ________ Volume , Temperature _________ Temperature , Volume __________

34. 6. Charles’s Law A balloonhas a volume of 15.5 L and is in a room at 20.0 C. The temperature drops to 7.00 C, what is the new volume? V1 = V2 T1 T2 15.5 L = V2 (20.0 C + 273) (7.00 C + 273)

35. 6. Charles’s Law Soda container has volume of 62.2L at 150 C. New volume is 24.4 L, What is the new temperature?

36. lussacs’s law OBJECTIVE: PRESSURE and TEMPERATURE

37. Lussac’s law Relationship between TEMPERATURE and PRESSURE when volume is constant

38. Lussac’s law P1 = Initial Pressure T1 = Initial Temperature P2 = Pressure After T2 = Temperature After

39. Lussac’s law Units P = kPa, atm T = change to Kelvin!

40. lussac’s law Pressure , Temperature ________ Temperature , Pressure ________ Pressure , Temperature _________ Temperature , Pressure __________

41. Which law does this graph represent?

42. Lussac’s law The pressure in a tire is 101 kPaat 10.0 C. What will be the pressure at 45.0 C? (T must be in K)

43. Lussac’s law The pressure in a soda bottle is 505 kPaat 20.0 C. What is the pressure if bottle is warmed to 65.0 C? (T must be in K)

44. Charles & Lussac’s law Summary & Review • What does Charles’s Law state about volume and temperature? • What does Lussac’s law state about pressure and temperature? • What units must temperature be for both laws? • How do you change C to K? • This year’s Superbowl winner claimed that their football “deflated” because the weather was too cold. Explain the cold weather would effect a football

45. avogadro’s law OBJECTIVE: VOLUME and MOLE

46. Avogadro’s law Relationship between VOLUME and MOLE at STP

47. Avogadro’s law Relationship between VOLUME and MOLE When Pressure AND Temperature is held constant

48. Avogadro’s law during STP STP = Standard Temperature & Pressure 0 °C and 1 atm

49. Avogadro’s law 1 mole = 22.4 L

50. 8. Avogadro’s law