States of matter practice test
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. / condensationb. / oxidation / d. / displacement reactions
____5.According to the kinetic-molecular theory, which substances are made of particles?
a. / gases only / c. / all matterb. / 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.b. / the forces that act between the particles.
c. / diffusion.
d. / the mass of the particles.
____7.According to the kinetic-molecular theory, particles of matter are in motion in
a. / gases only. / c. / solids, liquids, and gases.b. / gases and liquids only. / d. / solids only.
____8.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.
____9.Unlike in an ideal gas, in a real gas
a. / all particles move in the same direction.b. / all particles have the same kinetic energy.
c. / the particles cannot diffuse.
d. / the particles exert attractive forces on each other.
____10.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.
____11.Two gases have the same temperature but different pressures. The kinetic-molecular theory does not predict that
a. / molecules in both gases have the same average kinetic energies.b. / molecules in the low-pressure gas travel farther before they collide with other molecules.
c. / both gases have the same densities.
d. / all collisions of the molecules are elastic.
____12.According to the kinetic-molecular theory, which is the most significant difference between gases and liquids?
a. / the shapes of the particlesb. / the mass of each particle
c. / the distance between the particles
d. / the type of collision that occurs between particles
____13.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.
____14.What determines the average kinetic energy of the molecules of any gas?
a. / temperature / c. / container volumeb. / pressure / d. / molar mass
____15.Which is an example of gas diffusion?
a. / inflating a flat tireb. / the odor of perfume spreading throughout a room
c. / a cylinder of oxygen stored under high pressure
d. / All of the above
____16.By which process do gases take the shape of their container?
a. / evaporation / c. / adhesionb. / expansion / d. / diffusion
____17.If a gas with an odor is released in a room, it quickly can be detected across the room because it
a. / diffuses. / c. / is compressed.b. / is dense. / d. / condenses.
____18.Which substance has the lowest density?
a. / H2O(g) / c. / Hg(l)b. / H2O(l) / d. / Hg(g)
____19.The density of a substance undergoes the greatest change when the substance changes from a
a. / liquid to a gas. / c. / solid to a liquid.b. / liquid to a solid. / d. / a molecular solid to an ionic solid.
____20.According to the kinetic-molecular theory, how does a gas expand?
a. / Its particles become larger.b. / Collisions between particles become elastic.
c. / Its temperature rises.
d. / Its particles move greater distances.
____21.Diffusion between two gases occurs most rapidly if the gases are at
a. / high temperature and the molecules are small.b. / low temperature and the molecules are large.
c. / low temperature and the molecules are small.
d. / high temperature and the molecules are large.
____22.Which is an example of effusion?
a. / air slowly escaping from a pinhole in a tireb. / 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
____23.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.
____24.Why does the air pressure inside the tires of a car increase when the car is driven?
a. / Some of the air has leaked out.b. / The air particles collide with the tire after the car is in motion.
c. / The air particles inside the tire increase their speed because their temperature rises.
d. / The atmosphere compresses the tire.
____25.What is the process by which molecules of a gas randomly encounter and pass through a small opening in a container?
a. / diffusion / c. / distillationb. / osmosis / d. / effusion
____26.Under which conditions do real gases most resemble ideal gases?
a. / low pressure and low temperature / c. / high pressure and high temperatureb. / low pressure and high temperature / d. / high pressure and low temperature
____27.Which gases behave most like an ideal gas?
a. / gases composed of highly polar moleculesb. / gases composed of monatomic, nonpolar molecules
c. / gases composed of diatomic, polar molecules
d. / gases near their condensation temperatures
____28.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.
____29.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.
____30.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.
____31.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.
____32.The intermolecular forces between particles are
a. / weaker in solids than in liquids.b. / stronger in gases than in solids.
c. / equal in strength in gases and in liquids.
d. / stronger in liquids than in gases.
____33.Which best describes the particles of a liquid compared to those of a gas?
a. / less random / c. / colderb. / lower in density / d. / higher in energy
____34.The particles in a liquid are usually
a. / closer together and lower in energy than those in a solid.b. / farther apart and higher in energy than those in a gas.
c. / closer together and lower in energy than those in a gas.
d. / farther apart and lower in energy than those in a solid.
____35.Which of these best describes vaporization?
a. / the process by which a liquid changes to a gasb. / the process by which a solid changes to a gas
c. / Both (a) and (b)
d. / Neither (a) nor (b)
____36.Which term best describes the process by which particles escape from the surface of a nonboiling liquid and enter the gas state?
a. / sublimation / c. / surface tensionb. / evaporation / d. / aeration
____37.Which of the following causes particles in a liquid to escape into a gas state?
a. / high kinetic energy / c. / surface tensionb. / a freezing temperature / d. / the combining of liquids
____38.A solid forms when the average energy of a substance's particles
a. / increases. / c. / decreases then increases.b. / decreases. / d. / creates a random arrangement.
____39.Which of these can happen due to decreasing the average energy of a liquid's particles?
a. / vaporization / c. / a random arrangementb. / evaporation / d. / freezing
____40.Particles within a solid
a. / do not move. / c. / move about freely.b. / vibrate about fixed positions. / d. / exchange positions easily.
____41.Forces holding particles together are strongest in a
a. / solid. / c. / gas.b. / liquid. / d. / vapor.
____42.The energy of the particles in a solid is
a. / higher than the energy of the particles in a gas.b. / high enough to allow the particles to interchange with other particles.
c. / higher than the energy of the particles in a liquid.
d. / lower than the energy of the particles in liquids and gases.
____43.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.
____44.Solids have a definite volume because
a. / the particles do not have a tendency to change positions.b. / the particles are far apart.
c. / they can be easily compressed.
d. / the energy of the particles is high.
____45.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.
____46.The rate of diffusion in solids is very low because the
a. / particles are not free to move about.b. / surfaces of solids usually contact gases.
c. / attractive forces are weak.
d. / melting points are high.
____47.Which of the following properties do solids share with liquids?
a. / fluidity / c. / definite volumeb. / definite shape / d. / slow rate of diffusion
____48.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.
____49.The difference between crystalline and amorphous solids is determined by
a. / temperature changes.b. / pressure when the substances are formed.
c. / amount of order in particle arrangement.
d. / strength of molecular forces.
____50.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.
____51.Which of the following is an amorphous solid?
a. / ice / c. / graphiteb. / diamond / d. / glass
____52.Which of the following is not correct about crystalline solids?
a. / They can maintain a definite shape without a container.b. / They can exist as single crystals.
c. / Their particles are held in relatively fixed positions.
d. / They are geometrically irregular.
____53.Which of the following is a crystalline solid?
a. / a plastic milk container / c. / a glass bottleb. / a quartz rock / d. / a three-dimensional glass cube
____54.Which substance's solid state consists of covalent molecular crystals?
a. / salt / c. / sodiumb. / water / d. / diamond
____55.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. / metallicb. / covalent network / d. / covalent molecular
____56.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 patternb. / crystal lattice / d. / crystalline system
____57.Which of the following is not a property of covalent network crystals?
a. / high conductivity / c. / high melting pointb. / hardness / d. / brittleness
____58.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.
____59.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.
____60.If the temperature and surface area of a liquid remain constant,
a. / the liquid is not in equilibrium with its vapor.b. / no further evaporation occurs.
c. / the rate of evaporation remains constant.
d. / the rate of condensation is greater than the rate of evaporation.
____61.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.
____62.When does the concentration of a vapor decrease?
a. / when the rate of condensation decreasesb. / when the temperature remains constant
c. / when the liquid phase is warmed
d. / when the rate of condensation exceeds the rate of evaporation
____63.A liquid-vapor system at equilibrium is kept at constant temperature while the volume of the system is doubled. When equilibrium is restored,
a. / the concentration of vapor molecules has decreased.b. / the vapor pressure is the same as the original vapor pressure.
c. / the volume of the liquid has increased noticeably.
d. / the number of liquid molecules has increased.
____64.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.
____65.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.
____66.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.
____67.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.
____68.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.
____69.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.
____70.What is the critical pressure?
a. / the pressure at which all substances are solidsb. / 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
____71.According to the figure below, what is the most volatile substance shown?
a. / benzene / c. / tolueneb. / water / d. / aniline
____72.The equilibrium vapor pressure of a liquid is
a. / the same for all liquids.b. / measured only at 0C.
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.
____73.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.
____74.A volatile liquid
a. / has strong attractive forces between particles.b. / evaporates readily.
c. / has no odor.
d. / is ionic.
____75.The equilibrium vapor pressure of water is
a. / constant at all temperatures.b. / specific for any given temperature.
c. / unrelated to temperature.
d. / inversely proportional to the temperature.
____76.The equilibrium vapor pressure of a liquid increases with increasing temperature because
a. / the rate of condensation decreases.b. / the average energy of the particles in the liquid increases.
c. / the volume decreases.
d. / the boiling point decreases.
____77.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.
____78.Whenever a liquid changes to a vapor, it
a. / absorbs energy from its surroundings. / c. / is boiling.b. / is in equilibrium with its vapor. / d. / is condensing.
____79.What is the process of a substance changing from a solid to a vapor without passing through the liquid phase?
a. / condensation / c. / sublimationb. / evaporation / d. / vaporization
____80.At pressures greater than 1 atm, water will boil at
a. / a temperature higher than 100C. / c. / 100C.b. / a temperature lower than 100C. / d. / 4C.
____81.Why would a camper near the top of Mt. Everest find that water boils at less than 100C?
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.
____82.Glycerol boils at a slightly higher temperature than water. This reveals that glycerol's attractive forces are
a. / nonexistent. / c. / the same as those of water.b. / weaker than those of water. / d. / stronger than those of water.
____83.Diethyl ether's boiling point is about 35C at 1 atm. At 1.5 atm, what will be ether's approximate boiling point?
a. / –10C / c. / 40Cb. / 20C / d. / 100C
____84.During boiling, the temperature of a liquid
a. / remains constant. / c. / decreases.b. / increases. / d. / approaches water's boiling point.
____85.During the process of freezing, a liquid
a. / loses kinetic energy. / c. / gains potential energy.b. / loses potential energy. / d. / gains kinetic energy.
____86.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.
____87.At about what temperature does water reach its maximum density?
a. / 0C / c. / 4Cb. / 2C / d. / 6C
____88.When water is warmed from its freezing temperature to its temperature of maximum density, it
a. / contracts. / c. / maintains a constant volume.b. / expands. / d. / increases in weight.
____89.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.
____90.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 kJb. / 0.429 kJ / d. / 84.4 kJ
____91.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.)