CHM 2046C Module 7II:
Chapter 13 Sample Multiple Choice Test #1
1. If heat is added to ice and liquid water in a closed container, and after the addition of the heat there is still ice and liquid water remaining
|
a. |
the vapor
pressure of water will decrease. |
|
b. |
the temperature
will increase some. |
|
c. |
the temperature
will decrease some. |
|
d. |
the vapor
pressure of water will rise. |
|
e. |
the vapor
pressure of water will remain constant. |
2. A closed vessel contains an inert gas A at 500 mm of Hg and 60?C. What is the total pressure in mm of Hg inside the vessel after a few drops of liquid B are injected and a phase equilibrium is established at 60?C? The vapor pressure of liquid B at 60?C is 80 mm of Hg.
|
a. |
Cl. |
|
b. |
Si. |
|
c. |
N. |
|
d. |
C. |
|
e. |
|
3. The normal boiling point of a liquid
|
a. |
is above the
critical temperature. |
|
b. |
is at the triple
point temperature. |
|
c. |
is at one
atmosphere pressure. |
|
d. |
is usually below
the triple point temperature. |
|
e. |
is only when the
liquid and vapor are in equilibrium. |
4. The vapor pressure of a given liquid will increase if
|
a. |
the liquid is
moved to a container in which its surface is very much larger. |
|
b. |
the volume of the
liquid is increased. |
|
c. |
the volume of the
vapor phase is increased. |
|
d. |
the temperature
is increased. |
|
e. |
a more volatile
liquid is added to the given liquid. |
5. Which of the following indicates very strong intermolecular forces of attraction in a liquid?
|
a. |
A very low boiling point |
|
b. |
A very low critical temperature. |
|
c. |
A very low heat of vaporization. |
|
d. |
A very low vapor pressure. |
|
e. |
A very low surface tension. |
6. The compounds Br2 and ICl have almost identical molecular weights, yet ICl boils at 97?C and Br2 boils at 59?C. The best explanation for the difference is
|
a. |
ICl is an ionic compound and Br2 is covalent. |
|
b. |
ICl is a nonpolar molecule and Br2
is polar. |
|
c. |
ICl has a longer bond than that in Br2. |
|
d. |
ICl has a measurable dipole moment and Br2 does
not. |
|
e. |
ICl has a stronger bond than that in Br2. |
7. In some compounds the hydrogen atom is covalently bonded to one atom and simultaneously attracted to another atom in another molecule by an electrostatic interaction. This interaction can occur when hydrogen is bonded to
|
a. |
Cl. |
|
b. |
Si. |
|
c. |
N. |
|
d. |
C. |
|
e. |
|
8. Which of the following compounds would be expected to have the lowest boiling point?
|
a. |
CH3CH2CH2F |
|
b. |
CH3CH2CH2OH |
|
c. |
|
|
d. |
CH3CH2COOH |
|
e. |
CH3CH2CH2NH2 |
9. Which of the following
compounds is expected to have the highest boiling point?
|
a. |
CH3CH3 |
|
b. |
CH3CH2CH3 |
|
c. |
CH3OCH3 |
|
d. |
CH3CH2CH2Cl |
|
e. |
CH3CH2CH2Br |
10. Which of the following would be expected to have the highest heat of vaporization?
|
a. |
H2O |
|
b. |
NH3 |
|
c. |
PH3 |
|
d. |
AsH3 |
|
e. |
SbH3 |
11. In the phase diagram below,
the solid, liquid, and vapor phases are represented respectively by
|
a. |
O, M, N. |
|
b. |
O, N, M. O, N, M. |
|
c. |
N, O, M. |
|
d. |
N, M, O. |
|
e. |
M, N, O. |
12. From a consideration of the
phase diagram below, a change from point M to point N corresponds to
|
a. |
sublimation. |
|
b. |
condensation. |
|
c. |
evaporation. |
|
d. |
solidification. |
|
e. |
liquefaction. |
13. The sublimation of solid carbon dioxide, dry ice, is an example of
|
a. |
evaporation. |
|
b. |
a physical property. |
|
c. |
a chemical property. |
|
d. |
a chemical change. |
|
e. |
a physical change. |
14. The heat of sublimation of a compound equals
|
a. |
heat of fusion plus heat of vaporization. |
|
b. |
heat of ionization plus heat of crystallization. |
|
c. |
heat of vaporization minus heat of fusion. |
|
d. |
heat of vaporization plus heat of crystallization. |
|
e. |
heat of crystallization minus heat of vaporization. |
15. The critical point of carbon tetrachloride is 283?C and 45 atm pressure. Liquid carbon tetrachloride has a vapor pressure of 10.0 atm at 178?C. Which of the following statements must be true?
|
a. |
The normal boiling of CCl4
must be greater than 178?C. |
|
b. |
Liquid CCl4 can exist
at temperatures greater than 283?C if the pressure is greater than 45 atm. |
|
c. |
The triple point must be less
than 178?C. |
|
d. |
Liquid and solid can only be in
equilibrium at one temperature -- the freezing point. |
|
e. |
Vapor and liquid can only be in
equilibrium at one temperature -- the normal boiling point. |
16. Which of the following as solids has a crystal containing discrete (or separate) molecules?
|
a. |
NaCl |
|
b. |
CH 4 |
|
c. |
graphite |
|
d. |
diamond |
|
e. |
SiO2 |
17. Which of the following compounds would be expected to have the highest melting point?
|
a. |
LiCl |
|
b. |
CCl4 |
|
c. |
MgCl2 |
|
d. |
NCl3 |
|
e. |
OCl2 |
18. An atom that is shared equally between eight cubic unit cells is called
|
a. |
a corner atom. |
|
b. |
a face atom. |
|
c. |
a body-centered atom. |
|
d. |
an edge atom. |
|
e. |
a diagonal atom. |
19. Europium crystallizes in a body-centered cubic lattice. The number of europium atoms in a unit cell is
|
a. |
1 |
|
b. |
2 |
|
c. |
4 |
|
d. |
6 |
|
e. |
8 |
20. An ionic crystalline solid, MX2, has cubic unit cell. Which of the following arrangements of the ions is consistent with the stoichiometry of the compound?
|
a. |
M2+ ions at the
corners and at each face, 8 X- ions at the body centers. |
|
b. |
M2+ ions at each
face, X- ions at the corners. |
|
c. |
M2+ ions at the
corners, X- ions at the faces and 2 X- ions at the body
centers. |
|
d. |
4 M2+ ions at the
body centers, X- ions at the corners and at the face centers. |
|
e. |
M2+ ions at the
corners and at the face centers, 4 X- ions at the body centers. |
21. In UO2, the uranium
ions form a face-centered cubic lattice. The oxide ions occupy the tetrahedral
sites. The uranium ions occupy the faces and comers of the unit cell. The total
number of uranium ions and oxide ions per unit cell is
|
a. |
2 |
|
b. |
4 |
|
c. |
6 |
|
d. |
8 |
|
e. |
12 |
Question Instructions: Lithium
chloride crystallizes in a face-centered cubic structure. The unit cell length
is 5.14 x 10-8 cm. The chloride ions are touching each other along
the face diagonal of the unit cell. The lithium ions fit into the holes between
the chloride ions.
22. How many lithium ions are
there in this unit cell?
|
a. |
1 |
|
b. |
2 |
|
c. |
3 |
|
d. |
4 |
|
e. |
8 |
Question Instructions: Lithium
chloride crystallizes in a face-centered cubic structure. The unit cell length
is 5.14 x 10-8 cm. The chloride ions are touching each other along
the face diagonal of the unit cell. The lithium ions fit into the holes between
the chloride ions.
23. What is the mass of LiCl in a unit cell?
|
a. |
7.04 x 10-23 g |
|
b. |
1.41 x 10-22 g |
|
c. |
2.82 x 10-22 g |
|
d. |
4.22 x 10-22 g |
|
e. |
5.63 x 10-22 g |
Question Instructions: Lithium
chloride crystallizes in a face-centered cubic structure. The unit cell length
is 5.14 x 10-8 cm. The chloride ions are touching each other along
the face diagonal of the unit cell. The lithium ions fit into the holes between
the chloride ions.
24. What is the density of the
lithium chloride?
|
a. |
1.04 g/cc |
|
b. |
2.08 g/cc |
|
c. |
2.42 g/cc |
|
d. |
3.11 g/cc |
|
e. |
3.78 g/cc |
Question Instructions: Lithium
chloride crystallizes in a face-centered cubic structure. The unit cell length
is 5.14 x 10-8 cm. The chloride ions are touching each other along
the face diagonal of the unit cell. The lithium ions fit into the holes between
the chloride ions.
25. What is the radius of the
chloride ion?
|
a. |
1.29 x 10-8 cm |
|
b. |
1.82 x 10-8 cm |
|
c. |
2.23 x 10-8 cm |
|
d. |
2.56 x 10-8 cm |
|
e. |
2.76 x 10-8 cm |