1. 1520 mm Hg = ____ atms. Use your notes to find the equivalence line. Day 4 11-7

2. How does a cartesian diver work? Day 4 11-7

3. 1. Gases consist of large #s of tiny particles that are far apart relative to their size (each particle has mass) Kinetic-molecular Theory - Gases 2. Collisions between gas particles and between particles and container walls are elastic 3. Gas particles are in constant, rapid, random motion… they possess kinetic energy

4. Kinetic-molecular Theory - Gases 4. There are no forces of attraction or repulsion between gas particles 5. The average kinetic energy of gas particles depends on the temperature of the gas

5. cartesian divers Day 4 11-7

6. 33,600 mL of Helium = ____ atoms at STP Day 5 11-9

8. The Gas Laws Boyle’s Law: – Pressure-volume relationship – the volume of a fixed mass of gas varies inversely with the pressure at constant temperature Comparing conditions: P 1 V 1 = P 2 V 2 Boyle’s Law: Constant n and T P and V change

9. The Gas Laws Charles’ Law: – Volume-temperature relationship – the volume of a fixed mass of gas varies directly with the Kelvin temperature at constant pressure Comparing conditions: V 1 /T 1 = V 2 /T 2 Temperature decrease Charles’ Law: – Constant n and P T and V change

10. The Gas Laws Gay-Lussac’s Law: – Pressure- temperature relationship – the pressure of a fixed mass of gas varies directly with the Kelvin temperature at constant volume Comparing conditions: P 1 /T 1 = P 2 /T 2 Low T - Slow moving High T - Fast moving Temperature Increase Gay-Lussac’s Law: – Constant n and V T and P change

11. http://mc2.cchem.berkeley.edu/Java/molecules/index.html Increase pressure Temperature __________ Volume __________ Increase temperature Volume __________ Pressure __________ Increase volumeTemperature __________ Pressure __________ increasesdecreases increases decreases What happens if…? Constant VConstant T Constant VConstant P Constant T

12. The pressure exerted on a 3 L sample of gas is 600 mm Hg, if the pressure is decreased to 300 mm Hg what is the new volume? 1.Highlight important info. 2.Choose a law 3.Identify conditions as beginning (1) or ending (2) 4.Solve

13. P 1 V 1 = P 2 V 2 DAY 6 11-10 1. What is Boyle’s law? _____________ 2. Write a Boyle’s law problem in your notebook with the answer 3. Why are temperatures around zero kelvins bad for an ideal gas?

14. Review section 14.2 and complete #s 17-19, 22, 24, + 25 on page 463

15. Whose Law P 1 /T 1 = P 2 /T 2 P 1 V 1 = P 2 V 2 V 1 /T 1 = V 2 /T 2 Gay-Lussac’s Boyle’s Charles’

16. At 100 K a sample exerts a pressure of 2.026e5 Pa, if the pressure is decreased to 1.013e5 Pa what is the new temperature? What law do you use? __________________ Solve: Gay-Lussac’s: P 1 /T 1 = P 2 /T 2

17. 1. At 100 K and 1 atm a sample has a volume of 2L, if the gas expands to 6L what is the new temperature? Not in notes

18. Observe what happens. How could we get the egg back out without breaking it? EXPLAIN why the egg enters the flask.

19. Ideal gas law – mathematical relationship of pressure, volume, temperature, and the # of moles of a gas PV = nRT R = the ideal gas constant = 8.314 Page 454 table 13.2 L * kPa mol * K http://en.wikipedia.org/wiki/Gas_constant

20. What pressure in atms. is exerted by 0.325 mol of hydrogen gas in a 4.08 L container at 35°C? 1. Convert to Kelvins 2. Choose R 3. Solve 0.0821 atm- L/mol-K 8.314 J/mol-K PV = nRT

21. DAY 1 11-11 A sample of gas that contains 4.0 moles at 400K and 2 atms. takes up how much space?

22. 1. If a balloon is in this room (about 1 atm. and 300 K) and its volume is 0.40 L, how many moles of gas does it contain? On notes page 6

23. What mass of chlorine gas in grams is contained in a 10.0 L tank at 27°C and 3.50 atm of pressure? 101 g On notes page 5

24. What is the volume occupied by 4.67 moles of H 2 at 27.0 °C and 2.00 atm.? On notes page 6

25. Boyle’s Law Ideal Gas Kinetic Energy Mole Standard Temperature and Pressure Attract Volume-temperature relationship Absolute zero Charles’ Law Avogadro’s Law Pascal Precipitate Synthesis reaction

26. Homework # 1 Unit 4

27. At 300 K a sample of gas occupies 5 L, if the volume is decreased to 2 L what is the new temperature? V 1 /T 1 = V 2 /T 2

28. 1. Explain what happens at very low temperatures in terms of kinetic molecular theory. 2. List one of the 5 assumptions of kinetic molecular theory. 5-6

29. Read Section 12.1 (Kinetic Molecular Theory) and complete #s 8-11 + 13 on page 410

30. Homework Practice problems 1 + 2 on page 443 Practice Problems 4-6 on page 446 Practice Problems 8 + 9 on page 448 Periods 3 & 6 5-5

31. 1.Highlight important info. 2.Choose a law 3.Identify conditions as beginning (1) or ending (2) 4.Solve Boyle’s Law: Constant n and T P and V change