Deck 10: The Liquid and Solid States

Question 1

Three phases of water are shown in the figure. List the terms used to identify the phase changes indicated by the arrows.

A)A = sublimation, B = vaporization, C = freezing
B)A = condensation, B = sublimation, C = melting
C)A = freezing, B = vaporization, C = melting
D)A = deposition, B = vaporization, C = melting
E)A = deposition, B = sublimation, C = freezing

Answer 1

A = deposition, B = vaporization, C = melting

Question 2

The pictured change of state occurs at constant temperature even though heat is being added. Where does this change of state occur on the cooling curve?

A)AB
B)BC
C)CD
D)DE
E)EF

Answer 2

DE

Question 3

What phase change is occurring in the figure, and is it endothermic or exothermic?

A)melting; exothermic
B)freezing; endothermic
C)freezing; exothermic
D)melting; endothermic
E)sublimation; endothermic

Answer 3

sublimation; endothermic

Question 4

The pictured change of state occurs at constant temperature even though heat is being added. Where does this change of state occur on the cooling curve?

A)AB
B)BC
C)CD
D)DE
E)EF

Question 5

The pictured change of state occurs at constant temperature even though heat is being removed. Where does this change of state occur on the cooling curve?

A)AB
B)BC
C)CD
D)DE
E)EF

Question 6

Which of the following statements is correct?

A)At the melting point of a substance, the solid, liquid, and gas phases are all in equilibrium.
B)The freezing point and the melting point of a substance are the same.
C)There is no fundamental difference in the melting process for covalent substances and ionic substances.
D)In order for a substance to go from the gas phase to the liquid phase, it must absorb energy from the surroundings.
E)In order for a substance to go from the liquid phase to the gas phase, it must give off energy to the surroundings.

Question 7

From the vapor pressure curve of propane, it can be seen that the normal boiling point of propane is about ________.

A)−137ºC
B)−120ºC
C)−60ºC
D)−42ºC
E)0ºC

Question 8

The atmospheric pressure on Mount Everest is about 0.30 atm. From the vapor pressure curve of propane, it can be seen the boiling point of propane at this elevation is about ________.

A)−137ºC
B)−120ºC
C)−67ºC
D)−42ºC
E)0ºC

Question 9

Which of the following statements is correct?

A)When the temperature of a sample of liquid is increased, the molecules move faster, but there is no change in the vapor pressure of the sample.
B)The melting point of metallic sodium is 97.8ºC, so at a temperature of 25ºC, it is a liquid.
C)If you cook an egg on a mountain, it will require a short cooking time, due to the high elevation.
D)When liquids evaporate, it requires an input of energy from the surroundings, so the surroundings become warm.
E)Nitrogen gas has a boiling point of −196ºC, so if it is cooled to −200ºC, it condenses.

Question 10

Which of the following statements is correct?

A)The phase change from solid to liquid is exothermic.
B)Liquids boil at lower than normal temperatures in Death Valley, since it is below sea level.
C)A substance with a low boiling point would be expected to have a relatively low vapor pressure at a low temperature.
D)The phase change from liquid to gas is exothermic.
E)When a substance condenses, heat energy is given off.

Question 11

Which of the following statements is correct?

A)A liquid which has a high boiling point has a higher vapor pressure at a given temperature than a liquid with a low boiling point.
B)Liquids boil at higher temperatures in the mountains due to the higher altitude.
C)Evaporation is an exothermic process, since heat is given off when a substance vaporizes.
D)Since acetone (nail polish remover)evaporates more readily than water, one would assume that acetone has weaker intermolecular forces.
E)The phase change from solid to gas is exothermic.

Question 12

The pictured change of state occurs at constant temperature even though heat is being removed. Where does this change of state occur on the cooling curve?

A)AB
B)BC
C)CD
D)DE
E)EF

Question 13

Which of the molecular-level images in the figure shows the liquid and vapor phases in equilibrium in a closed container?

A)I, II, and III
B)none of the images
C)I
D)V
E)V and VI

Question 14

What phase transition is occurring between points D and E on the cooling curve?

A)melting
B)freezing
C)evaporation
D)sublimation
E)deposition

Question 15

Three phases of water are shown in the figure. List the terms used to identify the phase changes indicated by the arrows.

A)A = sublimation, B = vaporization, C = freezing
B)A = vaporization, B = condensation, C = melting
C)A = vaporization, B = deposition, C = melting
D)A = sublimation, B = condensation, C = freezing
E)A = condensation, B = sublimation, C = freezing

Question 16

What phase transition is occurring between points B and C on the cooling curve?

A)melting
B)condensation
C)evaporation
D)sublimation
E)deposition

Question 17

What phase transition is occurring between points D and E on the heating curve?

A)melting
B)freezing
C)evaporation
D)sublimation
E)deposition

Question 18

What phase change is occurring in the figure, and is it endothermic or exothermic?

A)melting; exothermic
B)freezing; endothermic
C)freezing; exothermic
D)melting; endothermic
E)condensation; endothermic

Question 19

From the vapor pressure curve of acetone, it can be seen that the normal boiling point of acetone is about ________.

A)-50ºC
B)0ºC
C)50ºC
D)55ºC
E)100ºC

Question 20

What phase transition is occurring between points B and C on the heating curve?

A)melting
B)condensation
C)evaporation
D)sublimation
E)deposition

Question 21

Calculate the amount of heat energy, in units of kilojoules, required to evaporate 35.0 g of ethanol, CH₃CH₂OH, at 78.4ºC, ethanol's boiling point. (The molar heat of vaporization of liquid ethanol is 3.86 × 10⁴ J/mol. The molar mass of ethanol is 46.07 g/mol.)

A)29.3 kJ
B)1.35 × 10³ kJ
C)1.10 × 10³ kJ
D)8.38 × 10² kJ
E)9.21 × 10⁻⁴ kJ

Question 22

Which of the following statements regarding intermolecular forces is incorrect?

A)An intermolecular force is an attractive force that operates between molecules.
B)Bonding forces are much stronger than intermolecular forces.
C)London dispersion forces occur in all atoms and molecules.
D)London dispersion forces are the result of permanent dipoles in atoms or molecules.
E)Molecules which have hydrogen bonded to F, O, or N can undergo hydrogen-bonding.

Question 23

The physical properties of a substance influenced by the strength of intermolecular forces include all of the following except

A)density.
B)boiling point.
C)surface tension.
D)melting point.
E)mass.

Question 24

The diagram represents the physical state of a substance. Where does this physical state occur on the heating curve?

A)AB
B)BC
C)CD
D)DE
E)EF

Question 25

Calculate the amount of heat energy required to convert 35.0 g of ice at -12.5°C to water at 24.0°C. (C_water = 4.184 J/g°C; C_ice = 2.03 J/g°C; molar heat of fusion of ice = 6.01 × 10³ J/mol)

A)8.88 × 10² J
B)1.17 × 10⁴ J
C)1.61 × 10¹⁰ J
D)3.51 × 10³ J
E)1.61 × 10⁴ J

Question 26

Which of the following is not an attractive force that acts between the individual molecules of CH₃OH?

A)London dispersion forces
B)dipole-dipole forces
C)hydrogen-bonding forces
D)covalent bonds
E)none of these is correct

Question 27

The diagram represents the physical state of a substance. Where does this physical state occur on the cooling curve?

A)AB
B)BC
C)CD
D)DE
E)EF

Question 28

The physical properties of a substance influenced by the strength of intermolecular forces include all of the following except

A)melting point.
B)boiling point.
C)viscosity.
D)vapor pressure.
E)mass.

Question 29

Which of the following substances is most likely to be a gas at room temperature and atmospheric pressure?

A)Ni
B)Hg
C)CO₂
D)C₇H₁₆
E)CBr₄

Question 30

Calculate the amount of heat energy required to evaporate 27.5 g of water at 100.0ºC. (molar heat of vaporization of liquid water = 4.07 × 10⁴ J/mol)

A)62.1 kJ
B)1.12 × 10³ kJ
C)2.02 × 10⁴ kJ
D)6.20 × 10⁷ kJ
E)1.22 × 10⁻² kJ

Question 31

Calculate the amount of heat energy required to evaporate 55.0 g of water at 100.0ºC. (molar heat of vaporization of liquid water = 4.07 × 10⁴ J/mol)

A)1.24 × 10² kJ
B)2.24 × 10³ kJ
C)4.03 × 10⁴ kJ
D)1.24 × 10⁸ kJ
E)2.43 × 10⁻² kJ

Question 32

Calculate the amount of heat energy, in units of kilojoules, required to melt 75.0 g of ice at 0.0ºC. (molar heat of fusion of ice = 6.01 × 10³ J/mol)

A)4.50 × 10² kJ
B)25.0 kJ
C)13.0 kJ
D)2.25 × 10³ kJ
E)4.50 × 10⁻¹ kJ

Question 33

Calculate the amount of heat energy, in units of kilojoules, required to convert 50.0 g of liquid ethanol, CH₃CH₂OH, at 25.5°C to gaseous ethanol at 92.0°C. (C_{ethanol liquid} = 2.44 J/g°C; C_{ethanol gas} = 1.42 J/g°C; molar heat of vaporization of liquid ethanol = 3.86 × 10⁴ J/mol. The boiling point of ethanol is 78.4°C and its molar mass is 46.07 g/mol.)

A)49.2 kJ
B)1.93 × 10³ kJ
C)0.862 kJ
D)1.35 × 10² kJ
E)2.67 kJ

Question 34

Which of the following substances is most likely to be a gas at room temperature and atmospheric pressure?

A)Cs
B)SO₂
C)I₂
D)CCl₄
E)Ni

Question 35

The diagram represents the physical state of a substance. Where does this physical state occur on the heating curve?

A)AB
B)BC
C)CD
D)DE
E)EF

Question 36

Calculate the amount of heat energy required to convert 55.0 g of water at 62.5ºC to steam at 124.0°C. (C_water = 4.184 J/g°C; C_steam = 2.02 J/g°C; molar heat of vaporization of liquid water = 4.07 × 10⁴ J/mol)

A)2.25 × 10³ kJ
B)1.23 × 10² kJ
C)0.862 kJ
D)1.36 × 10² kJ
E)2.67 kJ

Question 37

The diagram represents the physical state of a substance. Where does this physical state occur on the cooling curve?

A)AB
B)BC
C)CD
D)DC
E)EF

Question 38

Calculate the amount of heat energy required to melt 25.0 g of ice at 0.0°C. (molar heat of fusion of ice = 6.01 × 10³ J/mol)

A)1.50 × 10² kJ
B)8.34 kJ
C)4.33 kJ
D)7.50 × 10² kJ
E)1.50 × 10⁻¹ kJ

Question 39

Which of the following substances is most likely to be a gas at room temperature and atmospheric pressure?

A)I₂
B)Pb
C)Ar
D)CCl₄
E)C₈H₁₈

Question 40

Calculate the amount of heat energy required to convert 27.5 g of water at 62.5°C to steam at 124.0°C. (C_water = 4.184 J/g°C; C_ice = 2.03 J/gºC; C_steam = 2.02 J/g°C; molar heat of fusion of ice = 6.01 × 103 J/mol; molar heat of vaporization of liquid water = 4.07 × 10⁴ J/mol)

A)6.15 × 10⁴ kJ
B)1.23 × 10² kJ
C)4.31 × 10² kJ
D)67.8 kJ
E)1.33 kJ

Question 41

Which of the following molecules experience dipole-dipole forces?

A)NO
B)Cl₂
C)CH₄
D)SiH₄
E)all of these

Question 42

Rank the following substances in order of increasing intermolecular forces: Ar, H₂O, N₂, O₂

A)Ar < H₂O < N₂ < O₂
B)Ar < H₂O < O₂ < N₂
C)H₂O < N₂ < O₂ < Ar
D)N₂ < O₂ < Ar < H₂O
E)Ar < N₂ < O₂ < H₂O

Question 43

Which of the following has the highest boiling point?

A)H₂
B)H₂O
C)H₂S
D)H₂Se
E)H₂Te

Question 44

Rank the following substances in order of increasing boiling point: O₂, Ne, Ar, H₂

A)O₂ < Ne < Ar < H₂
B)O₂ < Ar < Ne < H₂
C)H₂ < Ne < Ar < O₂
D)H₂ < Ne < O₂ < Ar
E)Ar < O₂ < Ne < H₂

Question 45

Which of the following has the strongest London dispersion forces?

A)CH₄
B)CF₄
C)CCl₄
D)CBr₄
E)CI₄

Question 46

Rank the following substances in order of increasing boiling point: F₂, Ne, He, Cl₂

A)F₂ < Ne < He < Cl₂
B)F₂ < He < Ne < Cl₂
C)F₂ < Cl₂ < He < Ne
D)He < Ne < F₂ < Cl₂
E)Cl₂ < F₂ < Ne < He

Question 47

Rank the following substances in order of increasing boiling point: Cl₂, Ar, Ne, Br₂

A)Cl₂ < Ar < Ne < Br₂
B)Ar < Ne < Br₂ < Cl₂
C)Ne < Ar < Br₂ < Cl₂
D)Ne < Ar < Cl₂ < Br₂
E)Cl₂ < Br₂ < Ar < Ne

Question 48

Which of the molecules in the figure has hydrogen bonding in the pure liquid state?

A)I only
B)II only
C)III only
D)II and III
E)I and II

Question 49

Rank the following substances in order of increasing intermolecular forces: He, HF, F₂, Ne

A)He < HF < F₂ < Ne
B)He < HF < Ne < F₂
C)He < Ne < F₂ < HF
D)He < F₂ < Ne < HF
E)HF < Ne < F₂ < He

Question 50

Which of the following has the highest boiling point?

A)CH₄
B)CF₄
C)CCl₄
D)CBr₄
E)CI₄

Question 51

Which of the following substances can participate in hydrogen bonding?

A)SiH₄
B)CH₂Cl₂
C)H₂O
D)PH₃
E)both H₂O and PH₃

Question 52

Which of the following substances can participate in hydrogen bonding?

A)CH₄
B)CHCl₃
C)H₂S
D)NH₃
E)both H₂S and NH₃

Question 53

Which of the following has the highest vapor pressure at a given temperature?

A)CH₄
B)CF₄
C)CCl₄
D)CBr₄
E)CI₄

Question 54

Which of the following molecules experience dipole-dipole forces?

A)NO₂
B)CO₂
C)CBr₄
D)SO₃
E)F₂

Question 55

Which of the following has the highest boiling point?

A)H₂
B)HF
C)HCl
D)HBr
E)HI

Question 56

Which of the following substances is most likely to be a gas at room temperature?

A)CBr₄
B)F₂
C)Mn
D)C₆H₁₄
E)Sr

Question 57

Rank the following substances in order of increasing intermolecular forces: Ne, NH₃, H₂, O₂

A)Ne < NH₃ < H₂ < O₂
B)Ne < NH₃ < O₂ < H₂
C)NH₃ < O₂ < H₂ < Ne
D)O₂ < H₂ < Ne < NH₃
E)H₂ < Ne < O₂ < NH₃

Question 58

Which of the molecules in the figure has hydrogen bonding in the pure liquid state?

A)I only
B)II only
C)III only
D)II and III
E)I and II

Question 59

Which of the following substances can participate in hydrogen bonding?

A)CH₄
B)HF
C)CH₃COCH₃
D)SiH₄
E)all of these choices are correct

Question 60

Which of the following molecules experience dipole-dipole forces?

A)CO₂
B)SO₂
C)CCl₄
D)H₂S
E)both SO₂ and H₂S

Question 61

Which of the following statements regarding the solid state is incorrect?

A)Most polymers, such as rubbers and plastics, are amorphous.
B)Minerals, such as quartz and amethyst, are crystalline solids.
C)Solids normally do not flow.
D)The particles of a solid are held in a rigid, 3-dimensional array.
E)The arrangement of the particles in a crystal lattice is called space packing.

Question 62

Which of the following statements regarding intermolecular forces is incorrect?

A)Hydrogen bonding is the strongest of the intermolecular forces.
B)London dispersion forces increase with increasing molecular size.
C)Dipole-dipole forces are present in all atoms and molecules.
D)In order for a pure substance to participate in hydrogen bonding, it must have hydrogen bonded to F, O, or N.
E)Intermolecular forces are much weaker than bonding forces.

Question 63

Which choice correctly lists the intermolecular forces present in CH₃Br?

A)London forces only
B)London forces and dipole-dipole forces
C)London forces, dipole-dipole forces, and hydrogen bonding
D)dipole-dipole forces and hydrogen bonding
E)London forces and hydrogen bonding

Question 64

Which of the following statements regarding the solid state is incorrect?

A)Many metals follow a close-packing arrangement of their atoms, much like the way fruit is stacked in the grocery store.
B)The forces holding the particles together in a solid will affect their properties.
C)Network solids tend to have very high melting points.
D)Nonpolar molecular solids tend to be good conductors of heat and electricity.
E)Ionic solids tend to be brittle.

Question 65

Which of the following statements regarding the liquid state is incorrect?

A)Liquids are about 1000 times denser than gases.
B)Liquids are normally about 90-95% as dense as their corresponding solid.
C)The viscosity of a liquid is a measure of its resistance to flow.
D)Molecules with high intermolecular forces will have high surface tension.
E)Surface tension increases as temperature increases.

Question 66

Which of the following is not one of the classifications into which solids can be organized?

A)metallic
B)ionic
C)molecular
D)liquid crystals
E)network

Question 67

Which of the following statements regarding the solid state is incorrect?

A)Solids are not very compressible.
B)Solids have rigid shapes and definite sizes.
C)If a material solidifies in a partially disordered state, it is an amorphous solid.
D)Substances which solidify in a very orderly manner form crystalline solids.
E)Glass is an example of a crystalline solid.

Question 68

Select the pair of substances which has the one with the higher equilibrium vapor pressure at a given temperature listed first.

A)H₂O, H₂S
B)CH₃CH₂OH, CH₃OH
C)CH₃COCH₃, CH₃CH₂CH₂OH
D)NH₃, PH₃
E)Br₂, Cl₂

Question 69

A solid substance has a high melting point, is hard, brittle, and conducts electricity when molten. This substance is probably a(n)________ solid.

A)metallic
B)ionic
C)network
D)nonpolar molecular
E)polar molecular

Question 70

Which of the following statements regarding the liquid state is incorrect?

A)Detergents increase the surface tension of water, in order to help it stay in droplet form.
B)If ice were denser than liquid water, lakes would freeze from the bottom up.
C)In the summer, one would use a motor oil with a high viscosity rating to better lubricate the engine at high temperatures.
D)A liquid such as C₁₅H₃₂ would be expected to be more viscous than C₆H₁₄.
E)Water rises in a glass capillary tube due to the interactions between the water molecules and the glass.

Question 71

A solid substance has a moderate melting point, is fairly soft, and is a nonconductor. This substance is probably a(n)________ solid.

A)metallic
B)ionic
C)network
D)nonpolar molecular
E)polar molecular

Question 72

A solid substance has a very high melting point, is very hard, and is a nonconductor whether molten or solid. This substance is probably a(n)________ solid.

A)metallic
B)ionic
C)network
D)nonpolar molecular
E)polar molecular

Question 73

Which of the following statements regarding intermolecular forces is incorrect?

A)Hydrogen bonding is the strongest of the intermolecular forces for substances of similar molar mass.
B)London dispersion forces are present in all atoms and molecules.
C)Dipole-dipole forces increase with increasing molecular size.
D)Bonding forces are much stronger than intermolecular forces.
E)Hydrogen bonding is the reason for the abnormally high boiling point of water.

Question 74

Arrange the following substances in order of increasing boiling point: N₂, H₂, NH₃, PH₃

A)H₂ < N₂ < PH₃ < NH₃
B)N₂ < H₂ < PH₃ < NH₃
C)H₂ < N₂ < NH₃ < PH₃
D)N₂ < PH₃ < NH₃ < H₂
E)NH₃ < PH₃ < N₂ < H₂

Question 75

Which choice correctly lists the intermolecular forces present in CH₃NH₂?

A)London forces only
B)dipole-dipole forces only
C)London forces, dipole-dipole forces, and hydrogen bonding
D)dipole-dipole forces and hydrogen bonding
E)hydrogen bonding only

Question 76

Select the pair of substances which has the one with the higher equilibrium vapor pressure at a given temperature listed first.

A)H₂O, HCl
B)CH₃OH, CH₄
C)CH₃CH₂CH₂OH, CH₃COCH₃
D)AsH₃, PH₃
E)Cl₂, Br₂

Question 77

A solid substance has a high melting point, is hard, and is a good conductor of both heat and electricity. It is also malleable and ductile. This substance is probably a(n)________ solid.

A)metallic
B)ionic
C)network
D)nonpolar molecular
E)polar molecular

Question 78

Which choice correctly lists the intermolecular forces present in CH₄?

A)London forces only
B)London forces and dipole-dipole forces
C)London forces, dipole-dipole forces, and hydrogen bonding
D)dipole-dipole forces and hydrogen bonding
E)London forces and hydrogen bonding

Question 79

Arrange the following substances in order of increasing boiling point: CH₃OH, CH₄, CH₃CH₂OH, HOCH₂CH₂OH

A)CH₃OH < CH₄ < CH₃CH₂OH < HOCH₂CH₂OH
B)CH₄ < CH₃OH < CH₃CH₂OH < HOCH₂CH₂OH
C)CH₄ < CH₃OH < HOCH₂CH₂OH < CH₃CH₂OH
D)CH₃OH < CH₄ < HOCH₂CH₂OH < CH₃CH₂OH
E)HOCH₂CH₂OH < CH₃CH₂OH < CH₃OH < CH₄

Question 80

Which of the following statements regarding the liquid state is incorrect?

A)Liquid water is denser than ice (solid water).
B)The viscosity of a liquid is related to its intermolecular forces-the stronger the forces, the higher the viscosity.
C)As temperature increases, so will the viscosity of a liquid.
D)Substances with strong intermolecular forces have high surface tension.
E)Detergents interfere with the attractive forces among water molecules to lower the surface tension of the water.