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22. Differentiate between liquids and solids in terms of particle spacing,
     arrangement and motion.
    

24. Describe how it is possible for a molecule to leave the surface of a
     liquid and enter the gas phase even though the temperature of the
     liquid is below the boiling point.
    

26. Describe equilibrium in terms of a liquid-vapor system. Why is this
     situation referred to as a dynamic equilibrium?
    

28.What is the relationship between vapor pressure and intermolecular
     forces of attraction?
    

2. What is meant by the mean free path of a particle?
     

3. Explain how gas exerts pressure on its container.
    

4. For what purpose is a manometer used?
    

5. What is the value of standard atmospheric pressure in kPa?
    Select One 760 1 6.023 101.3 103.1

6. How does the increase in the average kinetic energy of a substance
     affect its temperature?
   

7. Convert the following temperatures as indicated:

8. Describe the difference in particle motion among the different states
     of matter?
    

9. Why are most ionic compounds solids at room temperature?
     

10. What is a crystal? What determines the properties of a crystal?
     

11. How do simple cubic, body-centered cubic, and face centered cubic
     unit cells differ in the physical arrangements of the particles?
    

13. How do amorphous materials differ from crystalline substances?
    

14. What is the relationship between a unit cell and a space lattice?
    

15. What is the freezing point of a substance?
     

16. Which type of Van der Waals forces hold CCl₄ in the liquid state? Select One Dipole-Dipole Dipole-Induced Dipole London Dispersion

17. Define boiling point in terms of vapor pressure.
     

18. What does the triple point on a phase diagram represent?
     

20. Compare ionic and molecular substances in terms of types of attractive forces that
     hold their particles together.
   

21. Describe Dipole-Dipole forces of attraction.
    

22. Which of the three forces is the strongest?

                ionic        dipole-dipole        London Dispersion

23. What is meant by the statement that a liquid and it's vapor, in a closed container,
     are in a state of equilibrium?
   

24. can solids have a vapor pressure? Select One Yes No What you talkin' 'bout Willis?

25. As the temperature of a liquid increases, what happens to the vapor pressure?
    

26. Use the above graph of the vapor pressure of water vs temperature to answer the
     following questions:

    (a) At what temperature does water boil at standard atmospheric pressure?

    (b) At what point is water only in the liquid phase?

    (c) At what point is water in the vapor phase?

    (d) At what point is liquid water in equilibrium with water vapor?

27. The critical point for ammonia is at 132 oC and a pressure of 5.5 x 103 kPa. The
     triple point is at -77.7 oC and a pressure of 6 kPa. The normal boiling point
     is -33.4 oC. Sketch the phase diagram for ammonia. Submit when you turn your
     test in.

28. use the phase diagram for water above to answer the following questions:

     (a) What is the normal boiling point for water?

     (b) Give coordinates for a point where water is only a liquid.

     (c) Give the coordinates for a point where liquid water is in equilibrium with
          its vapor phase.

     (d) Give the coordinates where water is only a vapor.

     (e) What will happen to the vapor at point D if it is cooled at a constant pressure?
         

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