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CHAPTER 10

CHAPTER 10. GASES. PHYSICAL CHARACTERISTICS OF GASES. PHYSICAL CHARACTERISTICS OF GASES. Expansion. PHYSICAL CHARACTERISTICS OF GASES. Expansion no definite shape or volume. PHYSICAL CHARACTERISTICS OF GASES. Expansion no definite shape or volume Fluidity.

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CHAPTER 10

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  1. CHAPTER 10 GASES

  2. PHYSICAL CHARACTERISTICS OF GASES

  3. PHYSICAL CHARACTERISTICS OF GASES • Expansion

  4. PHYSICAL CHARACTERISTICS OF GASES • Expansion no definite shape or volume

  5. PHYSICAL CHARACTERISTICS OF GASES • Expansion no definite shape or volume • Fluidity

  6. PHYSICAL CHARACTERISTICS OF GASES • Expansion no definite shape or volume • Fluidity ability to flow

  7. PHYSICAL CHARACTERISTICS OF GASES • Expansion no definite shape or volume • Fluidity ability to flow • Low Density

  8. PHYSICAL CHARACTERISTICS OF GASES • Expansion no definite shape or volume • Fluidity ability to flow • Low Density 1/1000 the density of a liquid or solid

  9. PHYSICAL CHARACTERISTICS OF GASES • Expansion no definite shape or volume • Fluidity ability to flow • Low Density 1/1000 the density of a liquid or solid • Compressibility

  10. PHYSICAL CHARACTERISTICS OF GASES • Expansion no definite shape or volume • Fluidity ability to flow • Low Density 1/1000 the density of a liquid or solid • Compressibility volumes can be greatly decreased

  11. PHYSICAL CHARACTERISTICS OF GASES • Expansion no definite shape or volume • Fluidity ability to flow • Low Density 1/1000 the density of a liquid or solid • Compressibility volumes can be greatly decreased • Diffusion

  12. PHYSICAL CHARACTERISTICS OF GASES • Expansion no definite shape or volume • Fluidity ability to flow • Low Density 1/1000 the density of a liquid or solid • Compressibility volumes can be greatly decreased • Diffusion spontaneous mixing of a gas

  13. PHYSICAL CHARACTERISTICS OF GASES • Expansion no definite shape or volume • Fluidity ability to flow • Low Density 1/1000 the density of a liquid or solid • Compressibility volumes can be greatly decreased • Diffusion spontaneous mixing of a gas depends on 1) speed, 2) size, and 3) attractive forces

  14. PHYSICAL CHARACTERISTICS OF GASES • Expansion no definite shape or volume • Fluidity ability to flow • Low Density 1/1000 the density of a liquid or solid • Compressibility volumes can be greatly decreased • Diffusion spontaneous mixing of a gas depends on 1) speed, 2) size, and 3) attractive forces • Effusion

  15. PHYSICAL CHARACTERISTICS OF GASES • Expansion no definite shape or volume • Fluidity ability to flow • Low Density 1/1000 the density of a liquid or solid • Compressibility volumes can be greatly decreased • Diffusion spontaneous mixing of a gas depends on 1) speed, 2) size, and 3) attractive forces • Effusion particles passing through a tiny opening

  16. PHYSICAL CHARACTERISTICS OF GASES • Expansion no definite shape or volume • Fluidity ability to flow • Low Density 1/1000 the density of a liquid or solid • Compressibility volumes can be greatly decreased • Diffusion spontaneous mixing of a gas depends on 1) speed, 2) size, and 3) attractive forces • Effusion particles passing through a tiny opening proportional to speed and mass

  17. KINETIC MOLECULARTHEORY

  18. KINETIC MOLECULARTHEORY • based on the idea that all particles of matter are constantly in motion

  19. KINETIC MOLECULARTHEORY • based on the idea that all particles of matter are constantly in motion • can be used to explain the properties of solids, liquids, and gases

  20. The Kinetic MolecularTheory of GASES

  21. The Kinetic MolecularTheory of GASES • Gases have large numbers of particles that are very far apart from each other.

  22. The Kinetic MolecularTheory of GASES • Gases have large numbers of particles that are very far apart from each other. 2. All collisions are elastic—no net loss of kinetic energy.

  23. The Kinetic MolecularTheory of GASES • Gases have large numbers of particles that are very far apart from each other. 2. All collisions are elastic—no net loss of kinetic energy. 3. Particles are in continuous, rapid, random motion.

  24. The Kinetic MolecularTheory of GASES • Gases have large numbers of particles that are very far apart from each other. 2. All collisions are elastic—no net loss of kinetic energy. 3. Particles are in continuous, rapid, random motion. 4. There are no forces of attraction or repulsion between particles.

  25. The Kinetic MolecularTheory of GASES • Gases have large numbers of particles that are very far apart from each other. 2. All collisions are elastic—no net loss of kinetic energy. 3. Particles are in continuous, rapid, random motion. 4. There are no forces of attraction or repulsion between particles. 5. The average kinetic energy of the particles is dependent upon the temperature of the gas.

  26. PHYSICAL CHARACTERISTICS OF GASES • Expansion no definite shape or volume • Fluidity ability to flow • Low Density 1/1000 the density of a liquid or solid • Compressibility volumes can be greatly decreased • Diffusion spontaneous mixing of a gas depends on 1) speed, 2) size, and 3) attractive forces • Effusion particles passing through a tiny opening proportional to speed and mass

  27. PHYSICAL CHARACTERISTICS OF GASES • Expansion (assumptions #3 & #4) no definite shape or volume • Fluidity ability to flow • Low Density 1/1000 the density of a liquid or solid • Compressibility volumes can be greatly decreased • Diffusion spontaneous mixing of a gas depends on 1) speed, 2) size, and 3) attractive forces • Effusion particles passing through a tiny opening proportional to speed and mass

  28. PHYSICAL CHARACTERISTICS OF GASES • Expansion (assumptions #3 & #4) no definite shape or volume • Fluidity (assumption #4) ability to flow • Low Density 1/1000 the density of a liquid or solid • Compressibility volumes can be greatly decreased • Diffusion spontaneous mixing of a gas depends on 1) speed, 2) size, and 3) attractive forces • Effusion particles passing through a tiny opening proportional to speed and mass

  29. PHYSICAL CHARACTERISTICS OF GASES • Expansion (assumptions #3 & #4) no definite shape or volume • Fluidity (assumption #4) ability to flow • Low Density (assumption #1) 1/1000 the density of a liquid or solid • Compressibility volumes can be greatly decreased • Diffusion spontaneous mixing of a gas depends on 1) speed, 2) size, and 3) attractive forces • Effusion particles passing through a tiny opening proportional to speed and mass

  30. PHYSICAL CHARACTERISTICS OF GASES • Expansion (assumptions #3 & #4) no definite shape or volume • Fluidity (assumption #4) ability to flow • Low Density (assumption #1) 1/1000 the density of a liquid or solid • Compressibility (assumption #1) volumes can be greatly decreased • Diffusion spontaneous mixing of a gas depends on 1) speed, 2) size, and 3) attractive forces • Effusion particles passing through a tiny opening proportional to speed and mass

  31. PHYSICAL CHARACTERISTICS OF GASES • Expansion (assumptions #3 & #4) no definite shape or volume • Fluidity (assumption #4) ability to flow • Low Density (assumption #1) 1/1000 the density of a liquid or solid • Compressibility (assumption #1) volumes can be greatly decreased • Diffusion (assumption #3) spontaneous mixing of a gas depends on 1) speed, 2) size, and 3) attractive forces • Effusion particles passing through a tiny opening proportional to speed and mass

  32. PHYSICAL CHARACTERISTICS OF GASES • Expansion (assumptions #3 & #4) no definite shape or volume • Fluidity (assumption #4) ability to flow • Low Density (assumption #1) 1/1000 the density of a liquid or solid • Compressibility (assumption #1) volumes can be greatly decreased • Diffusion (assumption #3) spontaneous mixing of a gas depends on 1) speed, 2) size, and 3) attractive forces • Effusion (assumption #3) particles passing through a tiny opening proportional to speed and mass

  33. Ideal vs. Real

  34. Ideal vs. Real • Ideal Gas: an imaginary gas that perfectly fits all the assumptions of the kinetic molecular theory

  35. Ideal vs. Real • Ideal Gas: an imaginary gas that perfectly fits all the assumptions of the kinetic molecular theory • Real Gas: does not behave completely according to the assumptions of the kinetic molecular theory

  36. Ideal vs. Real • Ideal Gas: an imaginary gas that perfectly fits all the assumptions of the kinetic molecular theory • Real Gas: does not behave completely according to the assumptions of the kinetic molecular theory Noble gases and nonpolar molecules behave more like ideal gases because their particles have such little attraction for each other.

  37. Ideal vs. Real • Ideal Gas: an imaginary gas that perfectly fits all the assumptions of the kinetic molecular theory • Real Gas: does not behave completely according to the assumptions of the kinetic molecular theory Noble gases and nonpolar molecules behave more like ideal gases because their particles have such little attraction for each other. All gases behave more ideally when they are at very high temperatures and very low pressures.

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