1 / 26

Chapter 4 - Gases

Chapter 4 - Gases. Movie – phase diagrams Kinetic Theory Pressure Measurement Units Unit Conversions Boyle & Charles Combined Gas Law. Movie – Phase Diagrams. Take home message: how gases move around distances between molecules Other

osric
Download Presentation

Chapter 4 - Gases

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chapter 4 - Gases • Movie – phase diagrams • Kinetic Theory • Pressure Measurement • Units • Unit Conversions • Boyle & Charles • Combined Gas Law

  2. Movie – Phase Diagrams • Take home message: • how gases move around • distances between molecules • Other • There is more information in the movie – it’s all chemistry. • Much of it is “common sense” with scientific labels.

  3. Kinetic Theory • Define Temperature • Define Source of Pressure • Relate Molecular Motion to Gas Behavior.

  4. Kinetic Theory – Define Temperature • Temperature relates to the speed of molecular motion. • Fast moving molecules = higher temp. • Solids vibrate • Liquids wiggle (movie) • Gases move in straight lines • Actually, temp. relates to kinetic energy which is mass times speed. • Fat molecules move slower at same temp. • Skinny molecules move faster • (Geo Metro vs. GMC Suburban)

  5. Kinetic Theory - Source of Pressure • Pressure is the force of gas atoms bouncing off the walls of a container. BIFF POW

  6. Kinetic Theory:Molecular Motion  Gas Behavior • Hit the wall = pressure • Gas collisions are perfect bounces. • T = Moving faster  P__ • T = moving slower  P__ • More molecules  P__ • Smaller Bottle  P__

  7. How do we measure pressure? • Definition: P = force area • Wall Barometer (Fig. 4.8) • air pushes on a diaphram against a spring • calibrate the scale • Manometer • Air pushes on a mercury column.

  8. Pressure Units

  9. Pressure Unit Conversions • We always get to convert these! • 1 atm  760 torr = 760 mmHg = 14.7 psi = 101.3 kPa • Forget about “bar”

  10. Vacuum • A vacuum is a truly empty space. • No gas molecules. • Pressure = 0.0000000 atm. • Real experiments can only get to 0.00000000000000001 atm or so.

  11. What is vacuum? • Vacuum- literally translated, the word describes the volume from which all the air has been totally removed. • However, so far nobody has succeeded in achieving such a condition. Scientifically the highest vacuum yet reached is in the range of 10-14 torr. This result has been achieved during a test by IBM Thomas J. Watson Research Center, New York, USA, October 1976, in a cryogene system where the temperature dropped to minus 269 °C. • Even at this low pressure thousands of gas molecules were detected per cm3. Also far out in space the presence of gas has been measured. http://www.busch.com.au/whatisvacuum.htm

  12. Absolute vs. Gauge • Bike Tires? 45 psi • Car Tire? • The psi values we use are usually relative to atmospheric pressure. • “Gauge” pressure means 1 atm + the reading. • “Absolute” means 0.000 atm + the reading • Actual pressure in bike tire is 45 psi + 14.7 psi = 59.7 psi! • Chemistry lab experiments use absolute pressure.

  13. Pressure - Volume • Boyles’ Law • Change the volume of a gas sample • See what the pressure does (graph it). • Avogadro’s Law • Trap different volumes of gas in the syringe. • See what the pressure does.

  14. Pressure – Volume Math • Boyle’s Law says that: PV = k, P= k/V • If you do 2 experiments: • 1st Experiment: 1.0 atm, 5.0 mL • 2nd Experiment: ? atm, 25.0 mL

  15. Pressure - Temperature • Charles’ Law says that:Pressure  Temperature • P T • P T • Double temperature  double pressure • Careful: • You have to use Kelvin units for temperature.

  16. Pressure – Temperature Math • Charles’ Law says that: P = kT, k = P/T • If you do 2 experiments: • 1st Experiment: 1.0 atm, 0 °C • 2nd Experiment: ? atm, 100 °C

  17. Combined Gas Law • We can shove Boyle & Charles together:

  18. Combined Gas Law - Math • These problems are all about setting them up right • At 56°C and 868 torr, a gas takes up 4.30 L. What will the pressure be if the volume is changed to 6.36 L and cooled to 12 °C? Case 1 Case 2 P _868 torr_ _???_____ V _4.30 L___ _6.36 L_ T _56°C=329K_ _12°C=285K_

  19. Combined Gas Law - Math • Once you make the table, fill into the big equation. • Answer: 508.4 torr

  20. Combined Gas Law - Math • Is out answer good? • P went down. • Sample was cooled. • Volume went up. • Sounds ok by kinetic theory…

More Related