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Kinetic Theory: The Microscopic Macroscopic Connection

Kinetic Theory: The Microscopic Macroscopic Connection. Ideal Gas Law Van der Waals Equation Distribution of Molecular Speeds. Reading Question. What is the name of the quantity represented as v rms ? . 1. random-measured-step viscosity 2. root-mean-squared speed

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Kinetic Theory: The Microscopic Macroscopic Connection

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  1. Kinetic Theory: The Microscopic Macroscopic Connection Ideal Gas Law Van der Waals Equation Distribution of Molecular Speeds

  2. Reading Question What is the name of the quantity represented as vrms? 1. random-measured-step viscosity 2. root-mean-squared speed 3. relative-mean-system velocity 4. radial-maser-system volume

  3. Reading Question What is the name of the quantity represented as vrms? 1. random-measured-step viscosity 2. root-mean-squared speed 3. relative-mean-system velocity 4. radial-maser-system volume

  4. Reading Question What additional kind of energy makes CV larger for a diatomic than for a monatomic gas? 1. Charismatic energy 2. Translational energy 3. Heat energy 4. Rotational energy 5. Solar energy

  5. Reading Question What additional kind of energy makes CV larger for a diatomic than for a monatomic gas? 1. Charismatic energy 2. Translational energy 3. Heat energy 4. Rotational energy 5. Solar energy

  6. Reading Question What’s new on the course web site? • A picture of me. • Your grades. • A new picture of big Al. • Study Guide for Exam #3. • None of the above.

  7. Reading Question In preparing for today’s class I spent about ___ hours reading, doing homework, or looking over my notes. • ½ • 1 • 1 ½ • 2 • 2 1/3 • 3 or more

  8. Kinetic Theory • Heat of Transformation Slope a heat capacity • Heat of fusion – the heat to transform a gram of substance from solid to liquid. Qf = + or - mLf • Heat of vaporization – the heat to transform a gram of substance from liquid to gas. Q a time Qv = + or - mLv • Sublimation – solid to gas

  9. Kinetic Theory • Heat of Transformation

  10. Kinetic Theory • Heat Capacity and Specific Heat

  11. Kinetic Theory • Specific Heat

  12. Kinetic Theory • Specific Heat for an Ideal Gas

  13. Kinetic Theory

  14. Student Workbook

  15. Student Workbook

  16. Student Workbook

  17. Student Workbook

  18. Student Workbook

  19. Student Workbook

  20. Kinetic Theory Rotational modes • Heat Capacity Vibrational modes

  21. Kinetic Theory Translational modes • Heat Capacity Rotational modes Equipartition of Energy: When a system is in thermodynamic equilibrium, the average energy per molecule is ½ kT per degree of freedom. Vibrational modes

  22. (1) (2) (3) (4) (5) Class Questions Which first-law bar chart describes the process shown in the pV diagram?

  23. (1) (2) (3) (4) (5) Class Questions Which first-law bar chart describes the process shown in the pV diagram?

  24. Class Questions Objects A and B are brought into close thermal contact with each other, but they are well isolated from their surroundings. Initially TA = 0°C and TB = 100°C. The specific heat of A is more than the specific heat of B. The two objects will soon reach a common final temperature Tf. The final temperature is 1. Tf > 50°C. 2. Tf = 50°C. 3. Tf < 50°C.

  25. Class Questions Objects A and B are brought into close thermal contact with each other, but they are well isolated from their surroundings. Initially TA = 0°C and TB = 100°C. The specific heat of A is more than the specific heat of B. The two objects will soon reach a common final temperature Tf. The final temperature is 1. Tf > 50°C. 2. Tf = 50°C. 3. Tf < 50°C.

  26. Kinetic Theory • The Ideal Gas Law • P pressure exerted by the gas • V volume of the gas • N number of molecules in the gas • T temperature of the gas • k = 1.38X10-23 J/K Boltzmann’s constant Most real gases obey this law with very slight deviations A mole is 6.022X1023 molecules. • R = NAk = 8.314 J/Kmole universal gas constant

  27. Kinetic Theory • Kinetic Theory of the Ideal Gas • The gas consists of a very large number of molecules, each with mass but with negligible size and no internal structure. • The molecules do not exert any force on each other except during a collision. This means that there is no potential energy. • The molecules are moving in random directions with a distribution of speeds that is independent of direction. • Collision with each other and the walls are elastic.

  28. Kinetic Theory • Kinetic Theory of the Ideal Gas The definition of pressure is Newton’s second law So we need the change in momentum

  29. Kinetic Theory • Kinetic Theory of the Ideal Gas Thus, we find for the force on the wall Now using this in the pressure we find

  30. Kinetic Theory • Kinetic Theory of the Ideal Gas But now

  31. Kinetic Theory • Kinetic Theory of the Ideal Gas

  32. Kinetic Theory

  33. Kinetic Theory

  34. Kinetic Theory

  35. Kinetic Theory

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  37. Kinetic Theory

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