PS11.CondensedStates

Basic Chemistry (Chapters 1-16)

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CHEMISTRY 2001 NAME PROBLEM SET #11: Condensed States of Matter DATE PERIOD READ CH. 9 WHILE SOLVING THESE PROBLEMS! 1. Define each of the following terms: a. kinetic energy b. kinetic theory c. temperature (It’s glossary time!) 2. In your own words, write the three assumptions of the kinetic theory of gases: (1) (2) (3) 3. Explain why we call liquids and solids “condensed” states of matter: 4. Why does evaporation lower the temperature of a liquid? 5. Explain why increasing the temperature of a liquid increases its rate of evaporation. 6. Use Figure 9.12 to determine the boiling point of each of these liquids: a. ethanoic acid at 27 kPa b. chloroform at 80 kPa c. ethanol at 53 kPa
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7. At the top of Mt. Everest, water boils at only 60 ° C. Use Figure 9.12 to estimate the atmospheric pressure at the top of this mountain. 8. Define the following terms:
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Unformatted text preview: a. phase diagram b. triple point 9. The temperature of the gas in an aerosol container is 0 ° C (273 K). To what new temperature must the gas be raised to increase the average kinetic energy of its molecules by a factor of 3? 10. Analogies . Choose the term that best completes the second relationship. a. temperature : thermometer :: atmospheric pressure : ____ (1) valve (2) barometer (3) volume (4) gauge b. education : knowledge :: vaporization : _____ (1) evaporation (2) water (3) gas (vapor) (4) condensation c. evolution : organisms :: kinetic theory : _____ (1) evaporation (2) water (3) gas (vapor) (4) condensation 11. In general, molecular solids have lower melting points than ionic solids. Why? 12. What is the difference between nematic, smectic, and cholesteric liquid crystals?...
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PS11.CondensedStates - a. phase diagram b. triple point 9....

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