CHM 2046C Pretest Homework Packet             Name: ____________________

Please complete the following pretest homework sections before you attempt the exam. This is homework. You grade it. This completed packet is due the day of the exam. You must show all work. Any mathematical type problem application must show work. No credit for just writing the answer. No credit for a section if the sample problem is shown and you leave any additional problems which do not show the answer blank.


Module Seven Part II: Intermolecular Forces & Liquids/Solids

______(01) P. Phase Diagrams

______(01) Q. Intermolecular Forces

______(01) Q1: Intermolecular Forces Physical Properties

______(02) R. Enthalpy Change with Phase Change

______(01) S. Discussion Questions-Chapter11 Jespersen

______(02) U. Clausius-Clapeyron Equation Calculation

______(02) V. Vapor Pressure Calculation

_____ (00)  T. Key Terms-Chapter 11


______(10) Total M7ii Homework Packet


Part P Phase Diagrams 01 points

Identify the points labeled on the

Phase Diagram of Water







_____________________B.              _____________________H


_____________________C.              _____________________I


_____________________D.              _____________________J


_____________________E.               _____________________K





Phase Diagram for Carbon Dioxide


















____________________  T.


____________________ U.


____________________ V.


____________________ W.




Reading  Reference: Jespersen 7th Section 11.7 pages 541-543
Phase Diagram Question 11.57-11.65 p 568
See Examples 11.3/11.4 p 543
Work Practice Exercises 11.12-11.14  Page 544
Extra Exercises  11.111-11.114 page 571




Module 7II Q Intermolecular Forces  1 Point


Describe the different type of interparticle forces that can occur between atoms, molecules, and ions. 








Distinguish the forces called intermolecular forces.







What forces are referred to as van der Waals forces?







Draw a flow chart or diagram to summarize these intermolecular forces and show an example.

(Use Table 11.3 page 5.24)



Type of Interaction 

Factors Responsible

For Interaction 

Approximate Energy (kJ/mol)















Hydrogen Bonding,






Dipole-induced dipole






Induced dipole-induced dipole

(London dispersion forces)






Reading Reference Jespersen 7th Section 11.1
See Example 11.1 Page 524




Module 7II Q1 Intermolecular Forces  1 Point


1.   Define:











Surface Tension















2.   Explain why when you use an alcohol swab before receiving a shot the skin feels cool?












    Reading Reference: Jespersen 7th  Section 11.2 pages 525-531
    Practice Exercise 11.4 page 531
    End of Chapter Exercises Questions 11.12-11.29 pages 566-7






Part R: Enthalpy Change with Phase Changes 2 points


You put 2.50 L of water in a soup pot at 100 oC  and the water slowly evaporates. How much heat must have been supplied to evaporate all the water from the pot. 

 Δ Hvap of water is +40.7 kJ/mole and

the density of water at 100oC is 0.958 g/mL














Suppose 60.0 g of water at 75oC is added to 120 grams of ice at 0oC,  How many grams of ice will melt and what will be the final temperature of the mixture?
he molar heat of fusion of water 6.01 kJ/mol and the specific heat of water is 4.18 J/g oC




















 Reading Reference Jespersen 7th  Section 11.3 and Section 11.6
 See Worked Example 11.2 Page 539
 Work Practice Exercises 11.10 and 11.11 Page 540
End of Chapter Exercises Questions 11.107-11.110  Pages 570-1




Part S: Discussion Questions 1 point


1.a. What is the Hydrogen Bond?







1.b. Describe the requirements for the Hydrogen Bond..







1.c. Draw a hydrogen bond between a water molecule and an ethanol (CH3CH2OH) molecule.









2a. Describe the process of dynamic equilibrium that exists between a liquid and its vapor in a closed container.











2.b. Why does a system in an open container never reach equilibrium?















3.a. What is the critical point?










3.b. Draw a vapor pressure curve for water and demonstrate the critical points












4.a. Describe the phenomenon of surface tension.











4.b. does water climb up the sides of glassware, while Mercury would not? Sketch/label tubing to show each

















Part U: Clausius-Clapeyron Equation Calculation   2 points

The Clausius-Clapeyron Equation is:



Calculate: ΔHovap

  1. Diethyl ether is a volatile, highly flammable organic liquid that today is mainl used as a solvent.  Calculate the enthalpy of vaporization (ΔHovap ) of diethyl ether, (C2H5)2O.
    Diethyl ether has vapor pressures of 57.0 torre and 534 torre at -22.8oC and 25.4oC respectively.    R =
    8.3145 J/K∙mol 










 Addition End of chapter exercises: #11.119 and 11.120 Page 571 (ΔHovap)


Calculate:  P2

  1. The vapor pressure of diethyl ether is 401 torre at 18oC, and the molar heat of vaporization (ΔHovap) is 26kJ/mole , Calculate the vapor pressure at 32oC!








Calculate: T2

  1. At what temperature would diethyl ether have a vaport pressure of 250 torre?









Addition End of chapter exercises: #11.117 and 11.118 Page 571 (P2)


Reading Reference: Jespersen 7th Section11.9  Pages 547-549
See Example 11.5 pages 548-549
Try Practice Exercises  11.17/11.18 page 549




Part V: Vapor Pressure Calculation          2 point


If 0.50 g of pure water is sealed in an evacuated 5.0 L flask and the whole assembly is heated to 60oC, will the pressure be equal to or less than the equilibrium vapor pressure at this temperature?


 If less what will be the pressure in the flask?














 What if you used 2.0 g of water? Under either set of conditions, is any liquid water left in the flask, or does all the water evaporate? (The equilibrium vapor pressure of water at 60oC is 149.4 torr)
























Addition End of chapter exercises: #11.36-11.41 pages 567-568

Reading Reference: Jespersen 7th Section 11.4  Pages 533-535
No Sample Exercises in Jespersen 7th text or additional problems



Module Seven Part T: Key Terms Chapter 11   0 Points


Fill in the blank with the word(s) which best fit the description:



__________________1.  The heat required to convert solid to a liquid at its melting point.




___________________2. The heat required to convert liquid to a gas at its boiling point.




___________________3. A pressure-temperature plot that shows the conditions under which a

                                        substances exits as a solid, liquid, and a gas.



___________________4. Refers to the conversion of a gas (vapor) to a liquid.




___________________5. The unique temperature and pressure at which the solid, liquid, and

                                        gaseous phases of a substance exists.



___________________6.  Is the passage of molecules of a liquid to the gaseous state.




___________________7. The temperature at which a solid melts.



___________________8. The highest temperature at which a liquid can coexist in equilibrium

                                       with its vapor.



___________________9. The temperature at which a liquid’s vapor pressure becomes equal to

                                         the prevailing atmospheric pressure.



___________________10. Pressure exerted by the vapor in dynamic equilibrium with a liquid.

    at a constant temperature




Reading Reference: Chapter 11 Summary pages 563-565