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WorksheetsStates of Matter
Total questions: 50
Worksheet time: 25mins
Name
Class
Date
1.
Amorphous solids have no definite melting point because
a)
their particles move around each other
b)
their particles are arranged randomly
c)
their particles are constantly changing positions
d)
their particles are tightly packed
2.
Which condition is necessary for most gases to behave nearly ideally?
a)
high temperature
b)
high pressure
c)
low expansion
d)
low compressibility
3.
If a gas with an odor is released in a room, it quickly can be detected across the room because it
a)
is dense
b)
is compressed
c)
diffuses
d)
condenses
4.
The temperature at which the vapor pressure of a substance equals atmospheric pressure is its
a)
critical point
b)
melting point
c)
boiling point
d)
triple point
5.
If energy as heat is removed, most liquids will eventually
a)
evaporate
b)
freeze
c)
diffuse
d)
burn
6.
The point on a phase diagram that indicates the temperature and pressure conditions at which the solid, liquid and vapor of the substance can coexist at equilibrium is known as the
a)
triple point
b)
critical point
c)
equilibrium point
d)
phase point
7.
Compared with nonpolar substances of comparable molecular mass, water's molar enthalpy of vaporization is
a)
equal
b)
higher
c)
similar
d)
lower
8.
Liquids are more ordered than gases because liquids have
a)
weaker intermolecular forces and greater mobility of the particles
b)
weaker intermolecular forces and lower mobility of the particles
c)
stronger intermolecular forces and greater mobility of the particles
d)
stronger intermolecular forces and lower mobility of the particles
9.
Equilibrium is characterized by
a)
opposing processes occurring at equal rates
b)
changes in physical states
c)
net change in the amount of substance in one phase
d)
an open system
10.
A phase diagram relates the state of matter, pressure, and
a)
mass
b)
weight
c)
temperature
d)
volume
11.
At pressures greater than 1 atm, water will boil at
a)
a temperature higher than 100oC
b)
100oC
c)
4oC
d)
a temperature lower than 100oC
12.
The movements of particles in solids can best be described as
a)
vibrational
b)
from point to point
c)
like a lattice
d)
not in motion
13.
Water forms roughly spherical drops because of
a)
surface tension
b)
capillary action
c)
viscosity
d)
fluidity
14.
The difference between crystalline and amorphous solids is determined by
a)
amount of order in particle arrangement
b)
pressure when the substances are formed
c)
strength of molecular forces
d)
temperature changes
15.
Why does the air pressure inside the tires of a car increase when the car is driven?
a)
The atmosphere compresses the tire.
b)
Some of the air has leaked out.
c)
The air particles collide with the tire after the car is in motion.
d)
The air particles inside the tire increase their speed because their temperature rises.
16.
The smallest portion of a crystal lattice that shows the three dimensional pattern of the entire lattice is called the
a)
unit cell
b)
crystal structure
c)
formula cell
d)
molecular structure
17.
When their is a small decrease in temperature, the average kinetic energy of the particles of a liquid
a)
increases
b)
decreases
c)
becomes zero
d)
is not changed
18.
If the particles in a smale of matter are attracted to each other but can move past each other easily, the matter is a
a)
solid
b)
plasma
c)
liquid
d)
gas
19.
A mixture of alcohol, water, oil, and glycerin is poured into a graduated cylinder. The liquids separate to form layers from top to bottom: alcohol, oil, water, and glycerin. Based on this observation, which liquid is the most dense?
a)
glycerin
b)
water
c)
oil
d)
alcohol
20.
Why doesn't water in lakes and ponds of temperate climates freeze solid during the winter and kill nearly all the living things it contains?
a)
ice floats
b)
water is colorless
c)
the molar enthalpy of fusion of ice is relatively low
d)
water contracts as it freezes
21.
Water's relatively high boiling point is the result of
a)
hydrogen bonding
b)
London forces
c)
covalent bonding
d)
ionic bonding
22.
The molar enthalpy of fusion for water is 6.009 kJ/mol. What quantity of energy is released when 264 g of liquid water freezes? (Molar mass of water is 18.02 g/mol.)
a)
2.44 kJ
b)
88.0 kJ
c)
1586 kJ
d)
792 kJ
23.
Above the critical temperature, a substance
a)
sublimes
b)
is explosive
c)
does not have a vapor pressure
d)
cannot exist in the liquid state
24.
How does the molar enthalpy of fusion of ice compare with the molar enthalpy of fusion of other solids?
a)
it is relatively small
b)
it is relatively large
c)
it is about the same
25.
The standard molar enthalpy of vaporization for water is 40.79 kJ/mol. What mass of steam is required to release 459 kJ of energy upon condensation? (Molar mass of water is 18.02 g/mol.)
a)
25.5 g
b)
0.624 g
c)
1039 g
d)
203 g
26.
Which of the following is a crystalline solid?
a)
a plastic milk container
b)
a quartz rock
c)
a glass bottle
d)
a three-dimensional glass cube
27.
When heated, a pure crystalline solid will
a)
melt at a temperature slightly above its freezing temperature
b)
gradually soften before it melts
c)
melt over a wide temperature range
d)
exhibit a sharply defined melting temperature
28.
An increase in pressure exerted on a liquid does not compress the liquid as much as the same increase in pressure compresses a gas because
a)
particles are more closely packed in liquids
b)
intermolecular forces are stronger in liquids
c)
liquids transmit pressure in all directions
d)
particles in liquids are in constant movement
29.
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 leave.
b)
The flames are hotter at that elevation.
c)
The atmosphere has less moisture.
d)
There is less atmospheric pressure than at sea level.
30.
By which process do gases take the shape of their container?
a)
diffusion
b)
adhesion
c)
expansion
d)
evaporation
31.
According to the kinetic-molecular theory, particles in a liquid
a)
vibrate only
b)
move around randomly and constantly
c)
are bound together in fixed positions
d)
are packed together in an orderly arrangement
32.
What is the reason for the relatively low density of ice?
a)
the high number of hydrogen bonds
b)
empty spaces between molecules
c)
the low molar mass of water
d)
the small size of hydrogen and oxygen atoms
33.
Which is an example of effusion
a)
oxygen and gasoline fumes mixing in an automobile carburetor
b)
helium dispersing into a room after a balloon pops
c)
air slowly escaping from a pinhole in a tire
d)
the aroma of a cooling pie spreading across a room
34.
Which of the following is not correct about crystalline solids?
a)
They can exist as single crystals.
b)
They can maintain a definite shape without a container.
c)
Their particles are held in relatively fixed positions.
d)
They are geometrically irregular.
35.
Which of the following is an amorphous solid?
a)
glass
b)
graphite
c)
ice
d)
diamond
36.
Surface tension does not account for which of the following phenomena?
a)
meniscus formation
b)
decreasing surface area
c)
ability to diffuse
d)
capillary action
37.
Which is an example of a noncrystalline solid?
a)
emerald
b)
glass
c)
ice
d)
quartz
38.
The three states of matter of a particular substance, in order of the strength of intermolecular forces from least to greatest, are
a)
gas, solid, liquid
b)
gas, liquid, solid
c)
liquid, solid, gas
d)
solid, liquid, ga
39.
Unlike in an ideal gas, in a real gas
a)
all particles have the same kinetic energy
b)
all particles move in the same direction
c)
the particles exert attractive forces on each other
d)
the particles cannot diffuse
40.
The process of changing from a solid to a gas is known as
a)
vaporization
b)
condensation
c)
sublimation
d)
deposition
41.
The amount of energy needed to melt one mole of a substance is its molar
a)
enthalpy of fusion
b)
entropy of fusion
c)
entropy of vaporization
d)
enthalpy of vaporization
42.
Diffusion is much slower in liquids than in gases because
a)
liquid particles are closer together
b)
liquids have surface tension
c)
liquid particles weigh more
d)
liquids exist at lower temperature
43.
Which choice represents the triple point?
a)
C
b)
A
c)
AD
d)
AB
44.
Which choice represents the normal boiling point?
a)
C
b)
A
c)
AD
d)
AB
45.
Which choice represents the liquid state?
a)
D
b)
AC
c)
E
d)
B
46.
Which choice represents the critical point?
a)
A
b)
C
c)
AB
d)
B
47.
Which choice represents the critical pressure?
a)
AC
b)
C
c)
AB
d)
B
48.
Which choice represents the solid phase?
a)
D
b)
E
c)
AB
d)
B
49.
Which choice represents the normal freezing point?
a)
AD
b)
A
c)
AB
d)
B
50.
Which choice represents the vapor?
a)
B
b)
D
c)
AB
d)
E
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