Multiple Choice
Identify the
letter of the choice that best completes the statement or answers the question.
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1.
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The
attractive forces in a liquid are a. | strong enough to prevent the particles from changing
positions. | b. | too weak to hold the particles in fixed
positions. | c. | more effective than those in a solid. | d. | too weak to
limit the movements of the particles. | | |
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2.
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What
is vaporization? a. | the process by
which a liquid changes to a gas | b. | the process by which a solid changes to a
gas | c. | both a and
b | d. | neither a nor
b | | |
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3.
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The
intermolecular forces between particles in a solid are a. | weaker than
those in a gas. | b. | too weak to hold the particles in fixed
positions. | c. | stronger than those in a liquid. | d. | of different
types than those in a liquid. | | |
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4.
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Which
of the following properties do solids share with liquids? a. | fluidity | c. | definite
volume | b. | definite shape | d. | slow rate of diffusion | | | | |
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5.
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What
type of crystal consists of positive metal cations surrounded by valence electrons that are donated
by the metal atoms and belong to the crystal as a whole? a. | ionic | c. | metallic | b. | covalent network | d. | covalent molecular | | | | |
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6.
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What
is the pattern of points that describe the arrangement of particles in the entire crystal
structure? a. | unit
cell | c. | crystal
lattice | b. | cube | d. | type of symmetry | | | | |
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7.
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Which
of the following statements about ionic crystals is NOT correct? a. | Their structure
consists of positive and negative ions arranged in a regular pattern. | b. | The strong
binding forces between the positive and negative ions in their structure give them certain
properties. | c. | Their ions can be monatomic or
polyatomic. | d. | They consist of molecules held together by intermolecular
forces. | | |
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8.
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A
system is in equilibrium when a. | no physical or chemical changes are
occurring. | b. | the physical changes counteract the chemical
changes. | c. | opposing physical or chemical changes occur at equal
rates. | d. | only physical changes are occurring. | | |
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9.
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If
the temperature of a closed liquid-vapor equilibrium system is raised, its vapor
pressure a. | decreases. | c. | remains the
same. | b. | increases. | d. | shows no correlation. | | | | |
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10.
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Why
would a camper near the top of Mt. Everest find that water boils at less than
100ºC? a. | There is greater
atmospheric pressure than at sea level. | b. | The flames are hotter at that
elevation. | c. | There is less atmospheric pressure than at sea
level. | d. | The atmosphere has less moisture. | | |
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11.
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At
its triple point, water can a. | have only three pressure values. | b. | exist in
equilibrium in three different phases. | c. | only be present as vapor. | d. | exist only as a
solid. | | |
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12.
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According to the figure above, what is the most volatile substance
shown? a. | benzene | c. | toluene | b. | water | d. | aniline | | | | |
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13.
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How
does the molar heat of fusion of ice compare with the molar heat of fusion of other
solids? a. | It is about the
same. | b. | It is relatively small. | c. | It is relatively
large. | d. | It is about the same as that of colorless
solids. | | |
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14.
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The
molar heat of vaporization of water is 40.79 kJ at 100ºC. What is the heat of vaporization of 1
g of water? a. | 40.79
J | c. | 500.
J | b. | 80.3
J | d. | 2.26
kJ | | | | |
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15.
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The
molar heat of fusion for water is 6.008 kJ/mol. How much energy would be required to melt 94.0 g of
ice? a. | 0.869
kJ | c. | 31.3
kJ | b. | 81.7
kJ | d. | 282.
kJ | | | | |
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16.
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Why
is ice less dense than liquid water?
a. | The molecules in liquid water can crowd together more compactly
than in ice. | c. | Liquid water
molecules are farther apart than the molecules in ice. | b. | Liquid water's
energy level is lower than that of ice. | d. | Liquid water has fewer chemical impurities than ice
has. | | | | |
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17.
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The
critical temperature of a substance is the
a. | temperature at which the vapor pressure of the liquid is equal
to the external pressure
| c. | temperature at
which the solid, liquid, and vapor phases are all in equilibrium
| b. | temperature at
which the vapor pressure of the liquid is equal to 760 mm Hg
| d. | lowest temperature above which a substance cannot be liquefied
at any applied pressure
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Short Answer
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18.
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What
do points E and F represent in the figure above?
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19.
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Explain what the curves AB, AC, and AD represent in the figure above.
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20.
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A. Identify the changes in processes indicated in the following
phase diagram.
For each change of state indicate whether the change is endothermic or
exothermic and the driving force that favors the process.
B. The
critical temperature of H2O is 647.6 K and the critical pressure is 217.7 atm. i).What
state of H2O would you expect at 650K and 10,000 atm? ii). What state would you expect at
645K and 220 atm?
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