1 / 58

Chapter 14 The Behavior of Gases

Chapter 14 The Behavior of Gases. Compressibility. The measure of how much the volume of matter decreases under pressure. Properties of a Gas. They are easy to compress. They expand to fill their containers. They occupy far more space than the liquids or solids from which they form.

Download Presentation

Chapter 14 The Behavior of 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 14The Behavior of Gases

  2. Compressibility The measure of how much the volume of matter decreases under pressure.

  3. Properties of a Gas • They are easy to compress. • They expand to fill their containers. • They occupy far more space than the liquids or solids from which they form.

  4. Variables that describe a Gas • The four variables and their common units: 1. pressure (P) in kilopascals(kPa) 2. volume (V) in Liters(L) 3. temperature (T) in Kelvin(K) 4. number of moles (n) (mol)

  5. Amount of Gas • When we inflate a balloon, we are adding gas molecules. • Increasing the number of gas particles increases the number of collisions • thus, the pressure increases • If temp. is constant- doubling the number of particles doubles pressure

  6. Pressure and the number of molecules are directly related • More molecules means more collisions. • Fewer molecules means fewer collisions.

  7. Common use? • Aerosol (spray) cans • gas moves from higher pressure to lower pressure • a propellant forces the product out • whipped cream, hair spray, paint

  8. 2. Volume of Gas • In a smaller container, molecules have less room to move. • Hit the sides of the container more often. • As volume decreases, pressure increases. (think of a syringe)

  9. 3. Temperature of Gas • Raising the temperature of a gas increases the pressure, if the volume is held constant. • The molecules hit the walls harder, and more frequently! • The only way to increase the temperature at constant pressure is to increase the volume.

  10. Homework Section: 14.1 Practice Problems Review Due: 3/17/06

  11. The Gas Laws • These will describe HOW gases behave. • Can be predicted by the theory. • Amount of change can be calculated with mathematical equations.

  12. Boyle’s Law • At a constant temperature, gas pressure and volume are inversely related. • As one goes up the other goes down P1 x V1= P2 x V2

  13. A balloon is filled with 25 L of air at 1.0 atm pressure. If the pressure is changed to 1.5 atm what is the new volume?

  14. P1 = 1 atm V1 = 25 L P2 = 1.5atm V2 = ? L

  15. P1 x V1 = V2 P2 1atm x 25L = V2 1.5atm P1 x V1= P2 x V2 16.7 L = V2

  16. A balloon is filled with 73 L of air at 1.3atm pressure. What pressure is needed to change the volume to 43L?

  17. P1 = 1.3atm V1 = 73 L P2 = ? atm V2 = 43 L

  18. P1 x V1 = P2 V2 1.3atm x 73L = P2 43 L P1 x V1= P2 x V2 16.7 L = V2

  19. V1 V2 T1 T2 = Charles’s Law • The volume of a gas is directly proportional to the Kelvin temperature, if the pressure is held constant.

  20. What is the temperature of a gas expanded from 2.5 L at 25 ºC to 4.1L at constant pressure? V1 = 2.5L T1 = 25ºC + 273 = 298K V2 = 4.1L T2 = ?ºC

  21. V1 V2 T1 T2 = T2 T1 x V2 V1 = T2 298K x 4.1L 2.5L = T2 = 488K = 216°C

  22. What is the final volume of a gas that starts at 8.3 L and 17ºC, and is heated to 96ºC? V1 = 8.3L T1 = 17ºC + 273 = 290K T2 = 96°C + 273 = 369K V2 = ?ºC

  23. V1 V2 T1 T2 = V1 x T2 V2 T1 = 8.3L x 369K V2 290K = V2 = 10.6L

  24. P1 P2 T1 T2 = Gay-Lussac’s Law • The temperature and the pressure of a gas are directly related, at constant volume.

  25. What is the pressure inside a 0.250 L can of deodorant that starts at 25 ºC and 1.2 atm if the temperature is raised to 100 ºC? P1 = 1.2atm T1 = 25ºC + 273 = 298K T2 = 100ºC + 273 = 373K P2 = ? atm

  26. P2 T2 P1 T1 = P2 (373K)(1.2atm) 298K = P1 P2 T1 T2 = P2 = 1.5 atm

  27. Combined Gas Law • The Combined Gas Law deals with the situation where only the number of molecules stays constant. • Formula: (P1 x V1)/T1= (P2 x V2)/T2 • This lets us figure out one thing when two of the others change.

  28. A 15 L cylinder of gas at 4.8 atm pressure and 25 ºC is heated to 75 ºC and compressed to 17 atm. What is the new volume? P1 = 4.8 atm V1 = 15 L T1 = 25ºC + 273 = 298K P2 = 17 atm V2 = ? L T2 = 75ºC + 273 = 348K

  29. P1 V1 P2 V2 T1 T2 = V2 P1 V1T2 P2 T1 = V1 (4.8 atm)(15L)(348K) (17 atm)(298K) = V1 = 4.9 L

  30. P1 V1 P2 x V2 x = T1 T2 • The combined gas law contains all the other gas laws! • If the temperature remains constant... Boyle’s Law

  31. P1 V1 P2 x V2 x = T1 T2 • The combined gas law contains all the other gas laws! • If the pressure remains constant... Charles’s Law

  32. P1 V1 P2 x V2 x = T1 T2 • The combined gas law contains all the other gas laws! • If the volume remains constant... Gay-Lussac’s Law

  33. Homework Section: 14.2 Practice Problems Review Due: 3/21/06

  34. Ideal Gases • We are going to assume the gases behave “ideally”- obeys the Gas Laws under all temp. and pres.

  35. Ideal Gases • An ideal gas does not really exist, but it makes the math easier and is a close approximation. • Particles have no volume. • No attractive forces.

  36. Ideal Gases • There are no gases for which this is true; however, • Real gases behave this way at high temperature and low pressure.

  37. The Ideal Gas Law #1 • Equation: P x V = n x R x T • Pressure times Volume equals the number of moles times the Ideal Gas Constant (R) times the temperature in Kelvin. • This time R does not depend on anything, it is really constant • R = 8.31 (L x kPa) / (mol x K)

  38. The Ideal Gas Law • We now have a new way to count moles (amount of matter), by measuring T, P, and V. We aren’t restricted to STP conditions P x V R x T n =

  39. Examples • How many moles of air are there in a 2.0 L bottle at 19 ºC and 747 mm Hg? • What is the pressure exerted by 1.8 g of H2 gas in a 4.3 L balloon at 27 ºC? • Samples 12-5, 12-6 on pages 342 and 343

  40. 6. Ideal Gas Law #2 • P x V = m x R x T M • Allows LOTS of calculations! • m = mass, in grams • M = molar mass, in g/mol • Molar mass = m R T P V

  41. Density • Density is mass divided by volume m V so, m M P V R T D = D = =

  42. Ideal Gases don’t exist • Molecules do take up space • There are attractive forces • Otherwise there would be no liquids formed

  43. Real Gases behave like Ideal Gases. • When the molecules are far apart • The molecules do not take up as big a percentage of the space • We can ignore their volume. • This is at low pressure

More Related