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ChemWiki: The Dynamic Chemistry E-textbook > Wikitexts > UC Davis > UCD Chem 2B > UCD Chem 2B: Larsen > Homework Problems > 13: Solutions and their Physical Properties > Team 4

Team 4

Table of Contents

Questions

1.      Define London Forces, Dipole-Dipole Interactions, and Hydrogen Bonding and give an example of each.

2.      If within a benzene molecule C6H6, a new atom replaces one of the hydrogen molecules and a new boiling point is determined, explain which of the following would have the highest boiling point and why.

a.      C6H6

b.      C6H5F

c.      C6H5I

d.      C6H5OH

3.      Define Viscosity and determine the change in viscosity in terms of a change of an increase in temperature.

4.      Explain what happens to Viscosity with an increase and decrease in temperature.

5.      Label the following as either a liquid or a gas when at room temperature.

a.      CH4

b.      C3H8

c.      Br

6.      Define intermolecular hydrogen bonding and give an example of it.

7.      How many water molecules can hydrogen bond to ethanol (C2H60)?

29.   Equilibrium of Chlorine is at 25 degrees C increasing to 50 degrees C. Given a 300 ml sample is measured and weighs .5 grams, initial pressure of 750 mmHg and the reacting pressure of 760mm Hg, find the vaporization pressure of Cl in mmHg.

39.   Ethanol has vapor pressures of 20 mmHg and 100mmHg at 50 C and 100 C respectively.  Given this information, use Clausius-Clapeyron Equation to calculate enthalpy of vaporization.

45.   Determine which of the following are liquids at room temperature

a.      CH3OH

b.      Hg

c.      C6H5COOH

47.   Given the element zinc, with an enthalpy of fusion at 7.35 kJ/mol and a melting point of 692.6K.  As well the zinc has a volume of 1000 cm^3.  How much heat is absorbed at the melting point of zinc?  Assume d=5.61 g/cm^3

49.   What is the state of matter of CO2 at room temp in a concealed box given a mass of 100g?

51.   Draw a phase diagram sample and then show the change on the graph when a drop in pressure is implemented at a constant temperature.

55.Use the phase diagram given as 12.5 in your textbook.  Which is likely to occur away from the earth’s surface…

a.      CO2

b.      HCl

c.      NH3

61.   Of the following substances, which would have a lower density?

a.      Diamond or Graphite

63.   Define the term of bonding scheme and state the purpose of them.

67.   Define Moh’s value scale and determine which of the following have the highest Moh’s value

a.      Zr, Si, Se

69.   How many arrangements are there for the closest packing of spheres?

71.   What is the simplest repeating unit in a crystalline solid?

73.   A molecule has a face-centered crystal structure with a radius of 100 pm.  Calculate the density of this unknown.

75.   Polonium has a distance of 200 pm to the nearest atom in the crystal structure.  Calculate the diameter and density of Po

77.   Define a body centered cubic unit cell

79.   Sketch the unit cell of CaF2.

83.   Based upon the data in the figure located in the textbook figure 8-9, what would be the type of unit cell taken in by Ag.

94.   If the coolant in a car requires 0.0855 kJ to evaporate C2H5OH and 0.55 kJ to evaporate the rest of the water in the coolant.  Based on this information, estimate if the spray of the coolant is effective.

 

Answers

CHAPTER 12

1. London Forces – Forces with slight dipole moment (weak force) F-F

    Dipole-Dipole Interaction- Interactions between bonds. Usually non-metal bonds. CO2

    Hydrogen Bonding – Bonding a species with a hydrogen atom. (Strong bond) HCl

   

2. C6H5OH would have the highest boiling point because the bonds are stronger than the other.

 

3. Viscosity is the ability to move across the surface of water. When the temperature increase, the viscosity decrease and vise versa.

 

4. Viscosity increase temperature decrease. Viscosity decrease temperature increase.

 

5.

a) gas

b) gas

c) liquid

 

6. Hydrogen bonding is when a hydrogen atom combines with a species that will increase the boiling point (HCl)

 

7. 6

 

29. -366.6kJ/mol

 

39.-32.2kJ/mol

 

45.

a) gas

b) liquid

c) gas

 

47. 630kJ

 

49. Gaseous state

 

51. See example in book chapter 12 figure 28 and 29.

 

55.

a) Not on surface

b) Not on surface

c) Not on surface

 

61. Graphite

 

63.  A bond scheme is a schematic to see the different bonds a species can create. It is helpful to see different bond schematics to determine whether it is an acid or a base.

 

67. Si. A scale to determine the hardness of the element.

 

69. 5

 

71. Small 3-dimensional unit

 

73. 15.6g/cm^3

 

75. Diameter = 150pm Density = 13.4g/cm^3

 

77. 8 Corners of a given atom x 1/8 of the given atom's unit cell) + 1 additional lattice point = 2 atoms

 

79. See textbook page 535-537

 

83. Face center Cubic

 

94. Most of the energy is going into the water therefore the coolant spray is effective.

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10:18, 2 Oct 2013

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