Chemistry 13.2 - PowerPoint PPT Presentation

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Chemistry 13.2

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  1. Chemistry 13.2

  2. The Nature of Liquids 13.2 • Hot lava oozes and flows, scorching everything in its path, and occasionally overrunning nearby houses. When the lava cools, it solidifies into rock. The properties of liquids are related to intermolecular interactions. You will learn about some of the properties of liquids.

  3. 13.2 A Model for Liquids • A Model for Liquids • What factors determine the physical properties of a liquid?

  4. 13.2 A Model for Liquids • Substances that can flow are referred to as fluids. Both liquids and gases are fluids.

  5. 13.2 A Model for Liquids • The interplay between the disruptive motions of particles in a liquid and the attractions among the particles determines the physical properties of liquids.

  6. 13.2 Evaporation • Evaporation • What is the relationship between evaporation and kinetic energy?

  7. 13.2 Evaporation • The conversion of a liquid to a gas or vapor is called vaporization. • When such a conversion occurs at the surface of a liquid that is not boiling, the process is called evaporation.

  8. 13.2 Evaporation • In an open container, molecules that evaporate can escape from the container.

  9. 13.2 Evaporation • In a closed container, the molecules cannot escape. They collect as a vapor above the liquid. Some molecules condense back into a liquid.

  10. 13.2 Evaporation • During evaporation, only those molecules with a certain minimum kinetic energy can escape from the surface of the liquid.

  11. Evaporation • Animation 15 • Observe the phenomenon of evaporation from a molecular perspective.

  12. 13.2 Vapor Pressure • Vapor Pressure • When can a dynamic equilibrium exist between a liquid and its vapor?

  13. 13.2 Vapor Pressure • Vapor pressure is a measure of the force exerted by a gas above a liquid.

  14. 13.2 Vapor Pressure • In a system at constant vapor pressure, a dynamic equilibrium exists between the vapor and the liquid. The system is in equilibrium because the rate of evaporation of liquid equals the rate of condensation of vapor.

  15. 13.2 Vapor Pressure • Vapor Pressure and Temperature Change • An increase in the temperature of a contained liquid increases the vapor pressure. • The particles in the warmed liquid have increased kinetic energy. As a result, more of the particles will have the minimum kinetic energy necessary to escape the surface of the liquid.

  16. 13.2 Vapor Pressure

  17. 13.2 Vapor Pressure • Vapor Pressure Measurements • The vapor pressure of a liquid can be determined with a device called a manometer.

  18. 13.2 Vapor Pressure • Manometer

  19. 13.2 Boiling Point • Boiling Point • Under what conditions does boiling occur?

  20. 13.2 Boiling Point • When a liquid is heated to a temperature at which particles throughout the liquid have enough kinetic energy to vaporize, the liquid begins to boil.

  21. 13.2 Boiling Point • The temperature at which the vapor pressure of the liquid is just equal to the external pressure on the liquid is the boiling point (bp).

  22. 13.2 Boiling Point • Boiling Point and Pressure Changes • Because a liquid boils when its vapor pressure is equal to the external pressure, liquids don’t always boil at the same temperature. • At a lower external pressure, the boiling point decreases. • At a higher external pressure, the boiling point increases.

  23. 13.2 Boiling Point • Altitude and Boiling Point

  24. 13.2 Boiling Point

  25. Boiling Point • Animation 16 • Relate vapor pressure and boiling point to intermolecular attractive forces.

  26. 13.2 Boiling Point • Normal Boiling Point • Because a liquid can have various boiling points depending on pressure, the normal boiling point is defined as the boiling point of a liquid at a pressure of 101.3 kPa.

  27. 13.2 Boiling Point

  28. 13.2 Section Quiz. • 13.2.

  29. 13.2 Section Quiz • 1. In liquids, the attractive forces are • very weak compared with the kinetic energies of the particles. • strong enough to keep the particles confined to fixed locations in the liquid. • strong enough to keep the particles from evaporating. • strong enough to keep particles relatively close together.

  30. 13.2 Section Quiz • 2. Which one of the following is a process that absorbs energy? • freezing • condensation • evaporation • solidifying

  31. 13.2 Section Quiz • 3. In a sealed gas-liquid system at constant temperature eventually • there will be no more evaporation. • the rate of condensation decreases to zero. • the rate of condensation exceeds the rate of evaporation. • the rate of evaporation equals the rate of condensation.

  32. 13.2 Section Quiz • 4. Where must particles have enough kinetic energy to vaporize for boiling to occur? • at the surface of the liquid • at the bottom of the container • along the sides of the container • throughout the liquid

  33. 13.2 Section Quiz • 5. The boiling point of a liquid • increases at higher altitudes. • decreases at higher altitudes. • is the same at all altitudes. • decreases as the pressure increases.

  34. END OF SHOW