1 / 15

Gases

Gases. Kinetic-Molecular Theory of Gases Notes#5. All particles are in constant motion. As temperature increases kinetic energy ?. As gas particles move apart the volume ?. increases. increases. Point Masses. Gas particles are treated as a point with no volume and no mutual attraction

wbattaglia
Télécharger la présentation

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. Gases Kinetic-Molecular Theory of Gases Notes#5

  2. All particles are in constant motion. As temperature increases kinetic energy ? As gas particles move apart the volume ? increases increases

  3. Point Masses • Gas particles are treated as a point with no volume and no mutual attraction • -this is because they’re so small compared to the distances between them.

  4. A theoretical gas with no volume and no attraction. A series of theories will be studied about ideal gases -standard pressure of 101.32 kPa -standard temperature of 0°C or 273K -standard conditions are abbreviated STP Ideal Gases

  5. Therefore: • Kinetic theory explains properties of gases based on a molecular view. • The assumptions are: • The molecules are in continuous, random motion. • A molecule has negligible volume. • The forces between molecules are negligible. • The average kinetic energy depends on the temperature.

  6. Four Gas Law Variables Are: • V = volume • P = pressure • T = temperature • n = number of particles • (Case is important)

  7. Units of pressure • SI unit is Pascal (Pa) • 1Pa = 1 N/m2 derived from force • 1atm = 760mm Hg = 760 torr = 101.3 kPa =14.7 psi • 1torr = 1 mm Hg

  8. Relates volume and pressure -gas exerts pressure on its container’s walls -pressure depends on *number of molecules *average kinetic energy of the molecules Pressure = P . . . . . . . . Boyle’s Law . .

  9. Relates volume and pressure -gas exerts pressure on its container’s walls -pressure depends on *number of molecules *average kinetic energy of the molecules Plunger applies pressure (now 2P). -As pressure doubles, volume becomes ½. -(note the same number of particles now occupying ½ the space) . . . . . . . . Boyle’s Law . . . . . . .

  10. Boyle’s Law PV=k *P=pressure *V= volume *k=constant Experiments happen at room temperature(about 25ºC.) We need to convert the results to STP. Boyle’s Law

  11. Since and then (substituting for k) Boyle’s Law

  12. Since and then (substituting for k) or Boyle’s Law

  13. Since and then (substituting for k) or Units pressure - kPa volume - cm3 Boyle’s Law

  14. V1= P1= V2= P2= Think: pressure goes from 87.6 kPa to 101.325 kPa so Volume should be________ than 242 cm3 Math: 242 cm3 87.6 kPa ? Problem: a gas is collected in a 242 cm3 container at 87.6 kPa. What is its volume at STP? 101.325 kPa

  15. so Note: 209 < 242cm3 Now do CMC 358: 1, 2, 3(a,c,e) and 4(a,c,e).

More Related