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States of Matter

States of Matter. Chapter 13. Chapter 13- The States of Matter. Gases- indefinite volume and shape, low density. Liquids- definite volume, indefinite shape, and high density. Solids- definite volume and shape, high density

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States of Matter

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  1. States of Matter Chapter 13

  2. Chapter 13- The States of Matter • Gases- indefinite volume and shape, low density. • Liquids- definite volume, indefinite shape, and high density. • Solids- definite volume and shape, high density • Solids and liquids have high densities because their molecules are close together.

  3. 13.3 Liquids and Solids Not fixed Not fixed Fixed Indefinite Definite Definite Relatively high Extremely low Medium Extremely low Relatively high Low does not flow flows flows rapid medium none

  4. Ideal Gas • Definition of a gas in ideal conditions. • It states: • Individual molecules have no mass. • Individual molecules have no volume. • No intermolecular force between molecules.

  5. Elastic Collisions Elastic collisions are defined as a collision in which no energy is lost. H and S Balls

  6. Inelastic Collisions Most collisions are inelastic. Inelastic collisions lose energy as heat and sound during the collision.

  7. The Kinetic Theory of GasesMakes three descriptions of gas particles

  8. The Kinetic Theory of GasesMakes three descriptions of gas particles

  9. The Kinetic Theory of GasesMakes three descriptions of gas particles

  10. The Kinetic Theory of GasesMakes three descriptions of gas particles

  11. The Kinetic Theory of GasesMakes three descriptions of gas particles

  12. The Kinetic Theory of GasesMakes three descriptions of gas particles

  13. The Kinetic Theory of GasesMakes three descriptions of gas particles

  14. The Kinetic Theory of GasesMakes three descriptions of gas particles

  15. The Kinetic Theory of GasesMakes three descriptions of gas particles

  16. The Kinetic Theory of GasesMakes three descriptions of gas particles • A gas is composed of particles • molecules or atoms • Considered to be hard spheres far enough apart that we can ignore their volume. • Between the molecules is empty space.

  17. The particles are in constant random motion. • Move in straight lines until they bounce off each other or the walls. • All collisions are perfectly elastic

  18. Kinetic Energy and Temperature • Temperature is a measure of the Average kinetic energy of the molecules of a substance. • Higher temperature faster molecules. • At absolute zero (0 K) all molecular motion would stop.

  19. Pressure • Pressure is the result of collisions of the molecules with the sides of a container. • A vacuum is completely empty space - it has no pressure. • Pressure is measured in units of atmospheres (atm). • It is measured with a device called a barometer. • Atmospheric Pressure • Collisions of atoms and molecules in air with objects

  20. Standard Atmospheric Pressure 14.7 pounds per square inch. 760 mm Hg = 760 torrs 1.01325 X 105 Pa = 101.325 kPa 1 atm

  21. Barometer • At one atmosphere pressure a column of mercury 760 mm high. 1 atm Pressure Column of Mercury Dish of Mercury

  22. Barometer • At one atmosphere pressure a column of mercury 760 mm high. • A second unit of pressure is mm Hg • 1 atm = 760 mm Hg • Third unit is the Pascal • 1 atm = 101.3 kPa 1 atm Pressure 760 mm

  23. STP: Standard Temperature and Pressure Standard Temperature 0C = 273 K

  24. Kelvin Temperature Scale Kelvins = Celsius + 273

  25. Three Variables Describe a Gas Average kinetic energy ≈ temperature in kelvins. Volume is measured in liters. Pressure is the force of the gas particles.

  26. Diffusion The process by which particles disperse from regions of higher concentration to regions of lower concentration

  27. Crystals A solid has a definite volume and a definite shape. True solid substances are crystals. Orderly repeating pattern called a crystal lattice Examples: salt, sugar, bismuth, ice

  28. Amorphous Solids Solids with no crystal structure Breaks into smaller pieces of varying shapes and sizes. Examples: glass, wax and obsidian

  29. Vapor Pressure and Boiling Point Evaporated particles create pressure in a closed container. Boiling point of a substance is the temperature at which its vapor pressure is equal to atmospheric pressure. Normal boiling point of a liquid is the temperature at which its vapor pressure is equal to 1 atm

  30. Same KE – different speed • Mass affects kinetic energy. • Less mass, less kinetic energy at the same speed • The smaller particles must have a greater speed to have the same kinetic energy. • Same temperature, smaller particles move faster

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