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

_____________________A.

_____________________B. _____________________H

_____________________C. _____________________I

_____________________D. _____________________J

_____________________E. _____________________K

_____________________F

_____________________G

Phase Diagram for Carbon Dioxide

_____________________M.

_____________________N.

_____________________O.

_____________________P.

_____________________Q.

_____________________R

_____________________S

____________________ T.

____________________ U.

____________________ V.

____________________ W.

Reading Reference: Jespersen 7^th 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)	Example
Ion-dipole
Dipole-dipole
Hydrogen Bonding, X—H…:Y
Dipole-induced dipole
Induced dipole-induced dipole (London dispersion forces)

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

Module 7II Q1 Intermolecular Forces 1 Point

1. Define:

Compressibility

Diffusion

Surface Tension

Wetting

Viscosity

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

Reading Reference: Jespersen 7^th 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 H_vap of water is +40.7 kJ/mole and

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

Suppose 60.0 g of water at 75^oC is added to 120 grams of ice at 0^oC, 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 7^th 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: ΔH^o_vap

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

Addition End of chapter exercises: #11.119 and 11.120 Page 571 (ΔH^o_vap)

Calculate: P₂

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

Calculate: T₂

3. 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 7^th 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 60^oC, 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 60^oC is 149.4 torr)

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

Reading Reference: Jespersen 7^th Section 11.4 Pages 533-535
No Sample Exercises in Jespersen 7^th 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