1 / 31

Kinetic Theory of Gases I

Kinetic Theory of Gases I. Ideal Gas. The number of molecules is large. The average separation between molecules is large. Molecules moves randomly. Molecules obeys Newton’s Law. Molecules collide elastically with each other and with the wall. Consists of identical molecules.

willa
Télécharger la présentation

Kinetic Theory of Gases I

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. Kinetic Theory of Gases I

  2. Ideal Gas The number of molecules is large The average separation between molecules is large Molecules moves randomly Molecules obeys Newton’s Law Molecules collide elastically with each other and with the wall Consists of identical molecules

  3. in K n:the number ofmolesin the ideal gas total number of molecules Avogadro’s number: the number of atoms, molecules, etc, in a mole of a substance: NA=6.02 x 1023/mol. The Ideal Gas Law R:the Gas Constant: R = 8.31 J/mol · K

  4. Force Pressure: Area Rate ofmomentum given to the surface Force: Momentum: momentum given by each collision times the number of collisions in timedt Pressure and Temperature Pressure:Results from collisions of molecules on the surface

  5. The number of collisions hitting an areaAin timedtis Average density The momentum given by each collision tothe surface Only molecules moving toward the surface hit the surface. Assuming the surface is normal to the x axis, half the molecules of speed vx move toward the surface. Only those close enough to the surface hit it in timedt, those within the distancevxdt

  6. Momentumin timedt: Force: Pressure: Not all molecules have the same

  7. is the root-mean-square speed Pressure: Average Translational Kinetic Energy:

  8. Pressure: From and Temperature: Boltzmann constant:

  9. From and Avogadro’s number Molar mass

  10. Pressure  Density x Kinetic Energy Temperature  Kinetic Energy

  11. Internal Energy For monatomic gas: the internal energy = sum of the kinetic energy of all molecules:

  12. p p isothermal V isothermal constant pressure constant pressure constant volume isothermal constant volume constant volume constant pressure V T T (d) Constant temperature Constant volume Constant pressure HRW 16P(5th ed.).Consider a given mass of an ideal gas. Compare curves representing constant-pressure, constant volume, and isothermal processes on (a) a p-V diagram, (b) a p-T diagram, and (c) a V-T diagram. (d) How do these curves depend on the mass of gas?

  13. (a) b 7.5 (b) Pressure (kN/m2) 2.5 a c (c) 1.0 3.0 HRW 18P(5th ed.).A sample of an ideal gas is taken through the cyclic process abca shown in the figure; at point a, T = 200 K. (a) How many moles of gas are in the sample? What are (b) the temperature of the gas at point b, (c) the temperature of the gas at point c, and (d) the net heat added to the gas during the cycle? (d) Cyclic process ∆Eint = 0 Volume (m3) Q = W = Enclosed Area= 0.5 x 2m2 x 5x103Pa = 5.0 x 103 J

  14. (a) (b) Since for 0.5 vrms for 2 vrms HRW 30E(5th ed.).(a) Compute the root-mean-square speed of a nitrogen molecule at 20.0 ˚C. At what temperatures will the root-mean-square speed be (b) half that value and (c) twice that value?

  15. (a) HRW 34E(5th ed.).What is the average translational kinetic energy of nitrogen molecules at 1600K, (a) in joules and (b) in electron-volts? (b) 1 eV = 1.60 x 10-19 J

  16. Kinetic Theory of Gases II

  17. the more molecules the more collisions the bigger the molecules the more collisions Mean Free Path Molecules collide elastically with other molecules Mean Free Path l: average distance between two consecutive collisions

  18. For constant volume: For constant pressure: The 1st Law of Thermodynamics: (Monatomic) Molar Specific Heat Definition:

  19. Constant Volume (Monatomic)

  20. Constant Pressure (Monatomic)

  21. 1st Law Adiabatic Process Ideal Gas Law (Q=0) Divide by pV:

  22. Ideal Gas Law

  23. Eachdegree of freedomhas associated with it an energy ofper molecules. Equipartition of Energy The internal energy of non-monatomic molecules includes alsovibrationaland rotationalenergies besides the translationalenergy.

  24. Monatomic Gases 3 translationaldegrees of freedom:

  25. Diatomic Gases 3 translationaldegrees of freedom 2 rotationaldegrees of freedom 2 vibrationaldegrees of freedom HOWEVER,differentDOFsrequire different temperatures to excite. At room temperature, only the first two kinds are excited:

  26. HRW 63P(5th ed.).Let 20.9 J of heat be added to a particular ideal gas. As a result, its volume changes from 50.0 cm3 to 100 cm3 while the pressure remains constant at 1.00 atm. (a) By how much did the internal energy of the gas change? If the quantity of gas present is 2.00x10-3 mol, find the molar specific heat at (b) constant pressure and (c) constant volume. (a) Constant pressure: W = p∆V

  27. (b) (c) HRW 63P(5th ed.).Let 20.9 J of heat be added to a particular ideal gas. As a result, its volume changes from 50.0 cm3 to 100 cm3 while the pressure remains constant at 1.00 atm. (a) By how much did the internal energy of the gas change? If the quantity of gas present is 2.00x10-3 mol, find the molar specific heat at (b) constant pressure and (c) constant volume.

  28. (a) Adiabatic HRW 81P(5th ed.).An ideal gas experiences an adiabatic compression from p =1.0 atm, V =1.0x106 L, T = 0.0 ˚C to p =1.0 x 105 atm, V =1.0x103 L. (a) Is the gas monatomic, diatomic, or polyatomic? (b) What is its final temperature? (c) How many moles of gas are present? (d) What is the total translational kinetic energy per mole before and after the compression? (e) What is the ratio of the squares of the rms speeds before and after the compression? Monatomic

  29. (b) HRW 81P(5th ed.).An ideal gas experiences an adiabatic compression from p =1.0 atm, V =1.0x106 L, T = 0.0 ˚C to p =1.0 x 105 atm, V =1.0x103 L. (a) Is the gas monatomic, diatomic, or polyatomic? (b) What is its final temperature? (c) How many moles of gas are present? (d) What is the total translational kinetic energy per mole before and after the compression? (e) What is the ratio of the squares of the rms speeds before and after the compression?

  30. (c) (Pay attention to the units) (d) For N/n = 1 HRW 81P(5th ed.).An ideal gas experiences an adiabatic compression from p =1.0 atm, V =1.0x106 L, T = 0.0 ˚C to p =1.0 x 105 atm, V =1.0x103 L. (a) Is the gas monatomic, diatomic, or polyatomic? (b) What is its final temperature? (c) How many moles of gas are present? (d) What is the total translational kinetic energy per mole before and after the compression? (e) What is the ratio of the squares of the rms speeds before and after the compression?

  31. (e) HRW 81P(5th ed.).An ideal gas experiences an adiabatic compression from p =1.0 atm, V =1.0x106 L, T = 0.0 ˚C to p =1.0 x 105 atm, V =1.0x103 L. (a) Is the gas monatomic, diatomic, or polyatomic? (b) What is its final temperature? (c) How many moles of gas are present? (d) What is the total translational kinetic energy per mole before and after the compression? (e) What is the ratio of the squares of the rms speeds before and after the compression?

More Related