1. Test Review
Chapter 17

2. Melting and Freezing
Which is defined as the temperature at which the particles move fast enough to slip past each other?

3. Vapor Equilibrium Define temperature.
Explain the dynamic equilibrium in a closed beaker containing water.

4. Vapor Equilibrium H2O(l) H2O(g)
Show an equation for the reversible change of water in the liquid state to water in the vapor state.
H2O(l) H2O(g)

5. Equilibrium Define Le Chatelier’s principle.
Explain how ice skating works according to Le Chatelier’s principle.

6. Changing State
Why do substances with strong intermolecular forces have low vapor pressures?
Define melting point.

7. Changing State Name the phase change in: Boiling Melting Subliming
Depositing

8. Changing State Name the phase change in: Freezing Condensing
Evaporating
Liquefaction

9. Changing State Define Boiling point. Define normal boiling point.
Define volatile.

10. Liquefaction What is the critical point?
Why would you want to liquefy a gas?

11. Boiling
At what temperature does water boil?
What is a phase diagram?

12. Vapor Pressure Chart
When the pressure is 90 kPa, what is the boiling point of CCl4?
What is the normal boiling point of each gas?

13. Heat Calculations
How much heat, in KJ, is needed to melt 5.67 grams of FeO? ΔHfus = 32.2 KJ/g
Watch the units of the constant………

14. Heat Calculations
How much heat, in KJ, is needed to change the temperature of 55.5 grams of water from 20OC to 99OC ?
The C of water = 4.18 J/gOC

15. Heat Calculations
How much heat, in KJ, is needed to boil 58.5 grams of water?
ΔHvap= 2260 J/g

16. Heat Calculations
A piece of unknown metal with a mass of 23.8 grams is heated to 100oC and dropped into 50.0 grams of water at 24.0oC. The final temp is 32.5oC. Find the C of the metal. C of water = 4.18 J/goC

17. Heat Calculations
A piece of copper with a mass of 50.0 grams is heated to 450oC and dropped into grams of water at 24.0oC. Find the final temperature.
C of water = 4.18 J/goC
C of copper = J/goC

18. Intermolecular Forces
List the following from weakest to strongest:
Hydrogen bonds
Covalent bonds
van der Waals forces
Dipole-dipole forces
London forces

19. Intermolecular Forces
Define:
London forces

20. Intermolecular Forces
Define:
Dipole-dipole forces

21. Intermolecular Forces
Define:
Hydrogen bonding

22. Intermolecular Forces
Explain the trend in this graph:

23. Intermolecular Forces
What properties of water can be attributed to hydrogen bonding?