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Chapter 10 Sample


Multiple Choice
Identify the choice that best completes the statement or answers the question.
 

 1. 
According to the kinetic-molecular theory, particles of matter
a.
are in constant motion.
c.
have different colors.
b.
have different shapes.
d.
are always fluid.
 

 2. 
According to the kinetic-molecular theory, gases condense into liquids because of
a.
gravity.
c.
forces between molecules.
b.
atmospheric pressure.
d.
elastic collisions.
 

 3. 
The kinetic-molecular theory explains the behavior of
a.
gases only.
c.
liquids and gases only.
b.
solids and liquids only.
d.
solids, liquids, and gases.
 

 4. 
Which process can be explained by the kinetic-molecular theory?
a.
combustion
c.
condensation
b.
oxidation
d.
displacement reactions
 

 5. 
According to the kinetic-molecular theory, which substances are made of particles?
a.
gases only
c.
all matter
b.
liquids only
d.
all matter except solids
 

 6. 
The kinetic-molecular theory explains the properties of solids, liquids, and gases in terms of the energy of the particles and
a.
gravitational forces.
c.
diffusion.
b.
the forces that act between the particles.
d.
the mass of the particles.
 

 7. 
An ideal gas is a hypothetical gas
a.
not made of particles.
b.
that conforms to all of the assumptions of the kinetic theory.
c.
whose particles have zero mass.
d.
made of motionless particles.
 

 8. 
A real gas
a.
does not obey all the assumptions of the kinetic-molecular theory.
b.
consists of particles that do not occupy space.
c.
cannot be condensed.
d.
cannot be produced in scientific laboratories.
 

 9. 
According to the kinetic-molecular theory, which is the most significant difference between gases and liquids?
a.
the shapes of the particles
b.
the mass of each particle
c.
the distance between the particles
d.
the type of collision that occurs between particles
 

 10. 
According to the kinetic-molecular theory, particles of an ideal gas
a.
attract each other but do not collide.
b.
repel each other and collide.
c.
neither attract nor repel each other but collide.
d.
neither attract nor repel each other and do not collide.
 

 11. 
Which is an example of gas diffusion?
a.
inflating a flat tire
b.
the odor of perfume spreading throughout a room
c.
a cylinder of oxygen stored under high pressure
d.
All of the above
 

 12. 
Which is an example of effusion?
a.
air slowly escaping from a pinhole in a tire
b.
the aroma of a cooling pie spreading across a room
c.
helium dispersing into a room after a balloon pops
d.
oxygen and gasoline fumes mixing in an automobile carburetor
 

 13. 
What happens to the volume of a gas during compression?
a.
The volume increases.
b.
The volume decreases.
c.
The volume remains constant.
d.
It is impossible to tell because all gases are different.
 

 14. 
Which gases behave most like an ideal gas?
a.
gases composed of highly polar molecules
b.
gases composed of monatomic, nonpolar molecules
c.
gases composed of diatomic, polar molecules
d.
gases near their condensation temperatures
 

 15. 
Two gases with unequal molar masses are injected into opposite ends of a long tube at the same time and allowed to diffuse toward the center. They should begin to mix
a.
in approximately five minutes.
b.
closer to the end that holds the heavier gas.
c.
closer to the end that holds the lighter gas.
d.
exactly in the middle.
 

 16. 
The intermolecular forces between particles in a liquid can involve all of the following except
a.
London dispersion forces.
c.
dipole-dipole attractions.
b.
hydrogen bonding.
d.
gravitational forces.
 

 17. 
The particles in both gases and liquids
a.
consist only of atoms.
b.
can change positions with other particles.
c.
can only vibrate in fixed positions.
d.
are packed closely together.
 

 18. 
The compressibility of a liquid is generally
a.
less than that of a gas.
c.
equal to that of a gas.
b.
more than that of a gas.
d.
zero.
 

 19. 
Which best describes the particles of a liquid compared to those of a gas?
a.
less random
c.
colder
b.
lower in density
d.
higher in energy
 

 20. 
Which of the following causes particles in a liquid to escape into a gas state?
a.
high kinetic energy
c.
surface tension
b.
a freezing temperature
d.
the combining of liquids
 

 21. 
The compressibility of solids is generally
a.
lower than the compressibility of liquids and gases.
b.
higher than the compressibility of liquids only.
c.
about equal to the compressibility of liquids and gases.
d.
higher than the compressibility of gases only.
 

 22. 
In general, most substances are
a.
least dense in the liquid state.
b.
more dense as gases than as solids.
c.
less dense as solids than as liquids.
d.
most dense in the solid state.
 

 23. 
Which of the following properties do solids share with liquids?
a.
fluidity
c.
definite volume
b.
definite shape
d.
slow rate of diffusion
 

 24. 
Which causes the high density of solids?
a.
The particles are more massive than those in liquids.
b.
The intermolecular forces between particles are weak.
c.
The particles are packed closely together.
d.
The energy of the particles is very high.
 

 25. 
Compared with a crystalline solid, the particles in an amorphous solid
a.
occur in a random pattern.
b.
occur in a definite, three-dimensional arrangement.
c.
consist of molecular sheets.
d.
have a more complex unit cell.
 

 26. 
Which of the following is a crystalline solid?
a.
a plastic milk container
c.
a glass bottle
b.
a quartz rock
d.
a three-dimensional glass cube
 

 27. 
Which 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
 

 28. 
What is the total three-dimensional array of points that describes the arrangement of the particles of a crystal called?
a.
unit cell
c.
diffraction pattern
b.
crystal lattice
d.
crystalline system
 

 29. 
Which of the following is not a property of covalent network crystals?
a.
high conductivity
c.
high melting point
b.
hardness
d.
brittleness
 

 30. 
If the rate of evaporation from the surface of a liquid exceeds the rate of condensation,
a.
the system is in equilibrium.
b.
the liquid is boiling.
c.
energy as heat is no longer available.
d.
the concentration of the vapor is increasing.
 

 31. 
Molecules at the surface of a liquid can enter the vapor phase only if
a.
equilibrium has not been reached.
b.
the concentration of the vapor is zero.
c.
their energy is high enough to overcome the attractive forces in the liquid.
d.
condensation is not occurring.
 

 32. 
When does the concentration of a vapor decrease?
a.
when the rate of condensation decreases
b.
when the temperature remains constant
c.
when the liquid phase is warmed
d.
when the rate of condensation exceeds the rate of evaporation
 

 33. 
When energy as heat is applied to a liquid-vapor system at equilibrium, a new equilibrium state will have
a.
a higher percentage of liquid.
c.
equal amounts of liquid and vapor.
b.
a higher percentage of vapor.
d.
all liquid.
 

 34. 
If the temperature of a liquid-vapor system at equilibrium is reduced, the
a.
concentration of the vapor will decrease.
b.
rate of evaporation will increase.
c.
equilibrium is unaffected.
d.
percentage of liquid in the system will decrease.
 

 35. 
If the temperature of a liquid-vapor system at equilibrium increases, the new equilibrium condition will
a.
have a lower concentration of vapor.
b.
have an increased vapor pressure.
c.
not have equal rates of condensation and evaporation.
d.
be larger in volume.
 

 36. 
The triple point of a substance is the temperature and pressure conditions at which
a.
density is greatest.
b.
states of a substance coexist at equilibrium.
c.
equilibrium cannot occur.
d.
kinetic energy is at a minimum.
 

 37. 
Above the critical temperature, a substance
a.
does not have a vapor pressure.
c.
cannot exist in the liquid state.
b.
sublimes.
d.
is explosive.
 

 38. 
What is the critical pressure?
a.
the pressure at which all substances are solids
b.
the pressure at which the attractive forces in matter break down
c.
the highest pressure under which a solid can exist
d.
the lowest pressure under which a substance can exist as a liquid at the critical temperature
 

 39. 
According to the figure below, what is the most volatile substance shown?

mc039-1.jpg
a.
benzene
c.
toluene
b.
water
d.
aniline
 

 40. 
The equilibrium vapor pressure of a liquid is
a.
the same for all liquids.
b.
measured only at 0°C.
c.
constant for a particular liquid at all temperatures.
d.
the pressure exerted by a vapor in equilibrium with its liquid at a given temperature.
 

 41. 
At a given temperature, different liquids will have different equilibrium vapor pressures because
a.
the energy of the particles is the same for different liquids.
b.
diffusion rates differ for the liquids.
c.
the attractive forces between the particles differ among liquids.
d.
they cannot all be in equilibrium at once.
 

 42. 
A volatile liquid
a.
has strong attractive forces between particles.
b.
evaporates readily.
c.
has no odor.
d.
is ionic.
 

 43. 
The equilibrium vapor pressure of a molten ionic compound is likely to be
a.
lower than that of ether.
c.
higher than that of volatile liquids.
b.
zero except when it is boiling.
d.
proportional to the volume.
 

 44. 
What is the process of a substance changing from a solid to a vapor without passing through the liquid phase?
a.
condensation
c.
sublimation
b.
evaporation
d.
vaporization
 

 45. 
At pressures greater than 1 atm, water will boil at
a.
a temperature higher than 100°C.
c.
100°C.
b.
a temperature lower than 100°C.
d.
4°C.
 

 46. 
During boiling, the temperature of a liquid
a.
remains constant.
c.
decreases.
b.
increases.
d.
approaches water's boiling point.
 

 47. 
How does the molar enthalpy of fusion of ice compare with the molar enthalpy 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.
 

 48. 
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.
Water is colorless.
b.
Ice floats.
c.
The molar enthalpy of fusion of ice is relatively low.
d.
Water contracts as it freezes.
 

 49. 
The molar enthalpy of fusion for water is 6.008 kJ/mol. What quantity of energy is released when 253 g of liquid water freezes? (Molar mass of water is 18.02 g/mol.)
a.
759 kJ
c.
2.33 kJ
b.
0.429 kJ
d.
84.4 kJ
 

 50. 
The standard molar enthalpy of vaporization for water is 40.79 kJ/mol. What mass of steam is required to release 500. kJ of energy upon condensation? (Molar mass of water is 18.02 g/mol.)
a.
221 g
c.
1130 g
b.
325 g
d.
1660 g
 



 
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