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Review: LIQUIDS & PHASE CHANGES

Review: LIQUIDS & PHASE CHANGES. solid to liquid . Melting. What phase of matter is “B”?. Pressure . A. B. C. Temperature . Liquid. ________is the gas phase of a substance normally solid or liquid at room temperature. Vapor. Freezing occurs by the release of _____. energy.

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Review: LIQUIDS & PHASE CHANGES

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  1. Review: LIQUIDS & PHASE CHANGES

  2. solid to liquid • Melting

  3. What phase of matter is “B”? Pressure  A B C Temperature  Liquid

  4. ________is the gas phase of a substance normally solid or liquid at room temperature • Vapor

  5. Freezing occurs by the release of _____ • energy

  6. Describe a volatile liquid in terms of its rate of evaporation. • Evaporates quickly

  7. ______ is the resistance of a liquid to flow • Viscosity

  8. What phase of matter is “A”? A Pressure  B C Temperature  Solid

  9. What is the normal boiling point of water? • 100C

  10. Melting occurs by energy being ______. • absorbed

  11. ____________ is the temperature and pressure at which all 3 states of matter are at equilibrium • Triple point

  12. _______shows how states of matter are affected by changes in temperature/pressure • Phase diagram

  13. solid to gas • Sublimation

  14. The triple point of this substance occurs at: • 5.2 atm & 216.6 K

  15. __________ is a dynamic condition in which two opposing physical or chemical changes occur at equal rates in a given closed system • Equilibrium

  16. ________ is the temperature at which equilibrium vapor pressure equals atmospheric pressure • Boiling point

  17. _______ is the pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature. • Equilibrium vapor pressure

  18. ____________ is the spontaneous mixing of two or more substances. • Diffusion

  19. When energy is added to a substance, the particles would move ___________ • Faster

  20. When does a liquid boil? • Equilibrium vapor pressure EQUALS atmospheric pressure

  21. When energy is taken away from a substance, the particles would move __________ • Slower

  22. What is the most abundant liquid? • Water

  23. _____________ is a force common to all liquids that tends to pull adjacent parts of a liquid’s surface together. • Surface tension

  24. List 2 examples of surface tension. • Meniscus • Droplets can form • Objects float • Capillary rise

  25. List a volatile substance • Rubbing alcohol • Nail polish remover • Gasoline • hairspray

  26. When a system at equilibrium is disturbed by application of a stress, it attains a new equilibrium position that minimizes the stress. This is known as ___________ • Le Chatelier’s Principle

  27. liquid to solid • Freezing

  28. C(s) + H2O(g) CO(g) + H2(g) If the concentration of H2O was increased, the system would shift to the ________ • Right

  29. How does a substance evaporate, if equilibrium vapor pressure is LOW? WHY? • SLOWLY! • B/c there are STRONG IM forces and requires MORE kinetic energy to become a vapor

  30. Describe a liquid in terms of particle spacing. • Particles are packed relatively closely together

  31. Describe a liquid in terms of particle motion. • Particles vibrate around MOVING points

  32. gas to liquid • Condensation

  33. Describe the general volume of a liquid and use KMT to explain. • Definite VOLUME- b/c particles are close together

  34. Describe the general shape of a liquid and use KMT to explain. • NO Definite SHAPE- b/c particles vibrate around moving points

  35. Describe a liquid-vapor system at equilibrium. • The number of particles leaving the liquid (vaporization) EQUAL the number of particles re-entering the liquid (condensation)

  36. gas to solid • Deposition

  37. What happens to the boiling point of liquids on top of Mt. Everest? WHY? • Boiling point is lower • B/c atmospheric pressure is lower

  38. liquid to gas • Vaporization

  39. What phase of matter is “C”? A Pressure  B C Temperature  Gas

  40. What is the difference between the IM forces during melting and freezing? • Melting = Less IM forces b/c more particle collisions • Freezing = MORE IM forces b/c particles are moving slower

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