Q of the Day

1. Q of the Day • Locate your Chapter # 3 Quest. • Calculate and record your % grade. • Did you meet your goal? Why or why not. • Study (preparation) Plan for next test? • Record your new goal: • - Average your first three tests (or quests) and improve by at least two! Day 6 11-18

2. Q of the Day 33,600 mL of Helium = ____ atoms at STP Day 1 11-19

3. Q of the Day DAY 2 11-20 P1V1 = P2V2 1. What is Boyle’s law? _____________ 2. Why are temperatures around zero Kelvins bad for an ideal gas?

4. LAB PERIODS 1 and 2 Day 2 11-20

5. Kinetic-molecular Theory - Gases 1. Gases consist of large #s of tiny particles that are far apart relative to their size (each particle has mass) 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

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

7. 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: P1V1 = P2V2 Boyle’s Law: Constant n and T P and V change

8. 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: V1/T1 = V2/T2 Charles’ Law: – Constant n and P T and V change Temperature decrease

9. 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: P1/T1 = P2/T2 Gay-Lussac’s Law: – Constant n and V T and P change High T - Fast moving Low T - Slow moving Temperature Increase

10. Practice • 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? • Highlight important info. • Choose a law • Identify conditions as beginning (1) or ending (2) • Solve

11. Notes – top of page 5 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: P1/T1 = P2/T2

12. Whose Law P1/T1 = P2/T2 P1V1 = P2V2 V1/T1 = V2/T2 Gay-Lussac’s Boyle’s Charles’

13. Lake Nyos Africa’s killer lakes: http://natgeotv.com/uk/killer-fog/videos/tragedy-at-lake-nyos http://www.youtube.com/watch?v=LcPg7HyTWnM&feature=related http://www.youtube.com/watch?v=ppbcl-MP76s

14. Assignment Lab Reports and Presentations are due on Wednesday 12-4 Postlabs are due on Friday 11-22 Review section 14.2 and complete #s 17-19, 22, 24, + 25 on page 463 - DUE WEDNESDAY 11-20

15. Q of the Day DAY 2 11-28 2. Write a Boyle’s law problem (word problem) in your notebook with the answer

16. Practice 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

17. PRELAB

18. LAB

19. Q of the Day Specifically explain what happened in Part A of your lab (it will help to get your lab out). *** This will be important for your lab report, presentation, or postlab! Day 4-11-30

20. PERIOD 1 LAB You have homework! Postlabs due next time we meet 12-7 Lab reports and presentations due Tuesday 12-11

21. PERIOD 3 LAB Postlabs due Tuesday 12-4 Lab reports and presentations due Friday 12-7

22. Q of the Day Describe Dalton’s law. Day 3 12-7

23. LAB You have homework! Postlabs due next time we meet 12-7 Lab reports and presentations due Tuesday 12-11

24. 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

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

26. Practice 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

27. 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

28. What is the volume occupied by 4.67 moles of H2 at 27.0 °C and 2.00 atm.? On notes page 6

29. 4 mols H2O 3.3 mols Cu(NO3)2 X = 4.4 mols H2O 3 mols Cu(NO3)2 3 mols Cu 63.5 g Cu 2.0 mols HNO3 X X = 48 g Cu 8 mols HNO3 1 mol Cu 1 mol H2 1 mol CH3OH 32 g CH3OH 4.0 g H2 X X X = 32 g CH3OH 2 g H2 2 mols H2 1 mol CH3OH 28.0 g CH3OH X 100 = 88% 32 g CH3OH 1 mol Cl2 4 mols Na X = 2 mols Cl2 2 mols Na

30. 1 mol Na3PO4 3 mols Ba(NO3)2 261 g Ba(NO3)2 3.50 g Na3PO4 X X X = 8.35 g Ba(NO3)2 164 g Na3PO4 2 mols Na3PO4 1 mol Ba(NO3)2 1 mol Ba3(PO4)2 1 mol Ba(NO3)2 602 g Ba3(PO4)2 6.4 g Ba(NO3)2 X X X = 4.9 g Ba3(PO4)2 1 mol Ba3(PO4)2 261 g Ba(NO3)2 3 mols Ba(NO3)2 5.00 g Ba3(PO4)2 X 100 = 102% 4.9 g Ba3(PO4)2

31. Q of the Day • Gas pressure is the result of … • What is STP (specifically)? Day 5 11-14

32. Kinetic-molecular Theory - Gases Ideal gas – an imaginary gas that perfectly fits all the assumptions of the kinetic-molecular theory

33. Q of the Day 1520 mm Hg = ____ atms. Use your notes to find the equivalence line. Day 6 11-15