3. VUONG-SCHMICK GAS, LIQUID, SOLID

4. READING BAROMETER:

5. Homework Problems & Questions Monday 12/12 Friday 12/16 Read Sections Intro, 10.1 – 10.4 & 10.7 Read Sections 10.5, 10.6 & 10.8 Chapter 10 1, 2,3, 4, 5 11, 14, 16, 18, 2246, 48, 49, 53, 56 24, 2657, 60, 63, 66 30, 32, 34, 36, 40, 4276, 77, 80 70, 72, 74  Additional Problems – At least one will appear on the test! o Chapter 10, #89, 94, 97, 107(a), 110(e)

6. Demo: Pepper water – Intermolecular forces Boil egg in a jar – Guy Lussac’s law Balloon in freezer/hot plate – Charles’ law Candle, water, container – Combine gas law Balloon – Avogadro’s law

7. Guy Lussac’s law: If the temperature of a container is increased, the pressure increases. If the temperature of a container is decreased, the pressure decreases. Why? – Suppose the temperature is increased. – This means gas molecules will move faster and they will impact the container walls more often. – This means the gas pressure inside the container will increase, since the container has rigid walls (volume stays constant). Gay-Lussac's Law is a direct mathematical relationship. – This means there are two connected values and when one goes up, the other also increases.

8. Review: Matter takes different forms States of matter: What are the differences?

9. Gases and gas pressure: Our atmosphere is made up of (primarily) _____, ____ and ____. What about CO 2 result from green house effect? Gas mixture is________ (homo/hetero) and are compressible, resulting from the fact that molecules in gases are _______ _______. Critical thinking: – Why is mixing and compressing possible for gases and not solids or liquids?

10. characteristics Gas exert a measureable pressure on walls of container Pressure = p p = F/A F = ma Unit F = newton (N) = kgm/s 2 unit P = pascal (Pa) = N/m 2 = kg/(ms 2 ) Atmospheric pressure = ____________________ (define) Other pressure units: mm Hg, atm, and torr

11. Mercury barometer: How does it work? Measure atm pressure by determine height of mercury column supported in a sealed glass tube. P = F/A = mass x acceleration – Using density of mercury and convert to get 101,325 Pa – So 1 atm = 760 mm Hg = 101325 Pa

13. How to measure gas pressure inside container? With an open-end manometer – Similar to mercury barometer

15. Practice: Typical atmospheric pressure on top of Mt. Everest is 265mm Hg, convert this value to pascals and to atm:

18. d 1 H 2 =d 2 H 1 Assume that you are using an open end manometer filled with mineral oil rather than mercury. What is the gas pressure in the bulb (in mmHg) if the level of mineral oil in the arm connected to the bulb is 237 mm higher than the level in the arm connected to the atmosphere and atmospheric pressure is 746 mmHg? (density of mercury is 13.6 g/mL and density of oil is 0.822 g/mL)

19. If the density of water is 1.00 g/mL and the density of mercury is 13.6 g/mL, how high a column of water (in meter) can be supported by standard atm pressure? (hint: 1 atm pressure can support column of Hg 0.760 m high)

20. What is the pressure (in atm) in a container of gas connected to a mercury filled, open end manometer if the level in the arm connected to the container is 24.7 cm higher than in the arm open to the atmosphere and atmospheric pressure is 0.975 atm? (hint: 1 atm/76.0 cmHg)

21. What is the pressure of the gas inside the following apparatus (in mmHg) if the outside pressure is 750 mmHg? Hint: 10mmHg/1cmHg

22. Gas law Review: Boyle: p 1 V 1 = p 2 V 2 Charles: Guy Lussac P 1 /T 1 = P 2 /T 2 pressure and temp of gas are directly related. Avogadro: volume of a gas at constant temperature and pressure is directly proportional to the number of moles of gas present. =