Deck 15: Gases, Liquids, and Solids

Question 1

Acetone,a highly volatile liquid,is placed in a closed container.The amount of liquid decreases,but eventually becomes stable.The volume of the closed space above the liquid is increased.The amount of liquid then...

A)May or may not change, but no prediction can be made without additional information about temperature
B)May or may not change, but no prediction can be made without additional information about the magnitude of the volume increase
C)Remains the same
D)Increases
E)Decreases

Answer 1

Decreases

Question 2

The total pressure exerted by the oxygen saturated with water vapor is 764 torr at a temperature at which water vapor pressure is 26 torr.Find the partial pressure of the oxygen.

A)0.0340 torr
B)29.4 torr
C)738 torr
D)790 torr
E)1.99 × 10⁴ torr

Answer 2

738 torr

Question 3

Predict the order in which boiling points of the following hydrides decrease (highest boiling point first,lowest last): PH₃,AsH₃,SbH₃ (As is atomic number 33; Sb is atomic number 51).

A)PH₃, AsH₃, SbH₃
B)AsH₃, SbH₃, PH₃
C)SbH₃, AsH₃, PH₃
D)PH₃, SbH₃, AsH₃
E)SbH₃, PH₃, AsH₃

Answer 3

SbH₃, AsH₃, PH₃

Question 4

Identify the most correct statement comparing intermolecular attractions (IMA)in the liquid and gaseous states of the same substance:

A)IMA are weaker in the gaseous state because the molecules are larger at the higher temperature
B)IMA are weaker in the gaseous state because the molecules are hotter
C)IMA are weaker in the gaseous state because molecules move at slower speeds
D)IMA are weaker in the gaseous state because molecules are so far apart
E)IMA are weaker in the gaseous state because the molecules fill their container

Question 5

Hydrogen gas can be collected by water displacement when magnesium reacts with hydrochloric acid.When the container is filled with the hydrogen gas,which of the following is true of the total pressure (P)inside the container?

A)
B)
C)
D)
E)P = atmospheric pressure

Question 6

Which of the following statements is correct?

A)Intermolecular forces are weaker in liquids than in gases because the particles are closer to each other
B)Smaller intermolecular distances in liquids result in stronger intermolecular forces, when compared to intermolecular distances and forces in gases
C)Compared to liquids, large distances between gaseous molecules yield large intermolecular attractions
D)The smaller the distance between molecules the smaller the intermolecular attractions, therefore attractions are weaker in liquids than gases
E)All statements are correct

Question 7

Acetone,a highly volatile liquid,is placed in an open container.The liquid disappears.The vapor pressure of the acetone in the open container...

A)is higher than the equilibrium vapor pressure
B)is lower than the equilibrium vapor pressure
C)is the same as the equilibrium vapor pressure
D)is equal to the vapor pressure of acetone in a closed container
E)cannot be compared to the equilibrium vapor pressure without more information

Question 8

In a gas mixture the partial pressure of helium is 225 torr,of neon,375 torr,and of argon,5 torr.What is the total pressure exerted by the mixture?

A)605 torr
B)4.22 × 10⁵ torr
C)It cannot be calculated without knowledge of container volume
D)It cannot be calculated without atmospheric pressure
E)It cannot be calculated without both container volume and atmospheric pressure

Question 9

Which of the following properties of liquids is the least affected by the strength of intermolecular forces?

A)vapor pressure
B)boiling point
C)heat of vaporization
D)density
E)viscosity

Question 10

With all other factors being equal,which of the following correctly lists intermolecular forces in order of increasing strength?

A)Dipole forces < Induced dipole forces < Hydrogen bonds
B)Induced dipole forces < Dipole forces < Hydrogen bonds
C)Hydrogen bonds < Dipole forces < Induced dipole forces
D)Dipole forces < Hydrogen bonds < Induced dipole forces
E)Induced dipole forces < Hydrogen bonds < Dipole forces

Question 11

Examine the structure shown below. Which of the following is the most important intermolecular forces experienced between this molecule and an identical molecule?

A)hydrogen bonds
B)dipole forces
C)induced dipole forces
D)a and c are about the same in this case.
E)b and c are about the same in this case.

Question 12

Compared to a substance with induced dipole forces,a substance with hydrogen bond generally has:

A)a higher normal boiling point and vapor pressure, but a lower heat of vaporization
B)a lower normal boiling point, but higher vapor pressure and heat of vaporization
C)higher heat of vaporization but lower normal boiling point and vapor pressure
D)a lower normal boiling point and heat of vaporization, but higher vapor pressure
E)lower vapor pressure, but higher normal boiling point and heat of vaporization

Question 13

Consider the open-ended manometer shown below.In this apparatus the arm on the right is open to the atmosphere and feels the full effect of atmospheric pressure.The pressure in the chemistry lab at the time of this experiment is 755 mm Hg.The flask contains O₂,N₂ and Ne. Which of the following correctly applies to this apparatus?

A)
B)
C)
D)
E)none of the above

Question 14

Select from the following the statement that is incorrect or contrary to the generalizations developed in the textbook.

A)The strength of induced dipole forces depends on the ease with which electron distributions can be polarized
B)Dipole forces are present in NF₃, but not in CF₄
C)The principal intermolecular forces in a straight chain hydrocarbon such as C₈H₁₈ are induced dipole forces
D)Intermolecular forces are usually stronger for substances that exhibit hydrogen bonding than for otherwise similar substances lacking hydrogen bonds
E)Induced dipole forces exist in both polar and nonpolar molecular substances, but they are essentially the only attractions in polar compounds

Question 15

Draw the Lewis diagrams of CH₃OH and water,then from the Lewis diagrams,identify the statement among the following that is most apt to be incorrect.

A)Hydrogen bonds are probably the principal intermolecular force in both compounds
B)Both compounds have both hydrogen bonding and induced dipole forces
C)Both molecules being polar, dipole-dipole forces are present in both compounds
D)Induced dipole forces are present in CH₃OH, but not water
E)Induced dipole forces are probably the least significant intermolecular forces in both compounds

Question 16

Considering the molecular mass and polarity influences on physical properties,which of the following predictions about the boiling points of elemental bromine and chlorine fluoride is most apt to be correct?

A)Both molecular mass and polarity predicts Br₂ has the lower boiling point
B)Both molecular mass and polarity predicts Br₂ has the higher boiling point
C)Molecular mass predicts Br₂ has the lower boiling point, but molecular polarity predicts it has the lower boiling point
D)Molecular mass predicts Br₂ has the higher boiling point, but molecular polarity predicts it has the lower boiling point
E)Molecular mass and polarity have an insignificant influence on the physical properties of these molecules

Question 17

Acetone,a highly volatile liquid,is placed in a closed container.The amount of liquid decreases,but eventually becomes stable.At that time...

A)the rate of evaporation is equal to the rate of condensation
B)the rate of evaporation is less than the rate of condensation
C)the rate of evaporation is greater than the rate of condensation
D)the rates of evaporation and condensation cannot be compared without more information
E)the kinetic energy of each gaseous molecule is equal to the kinetic energy of each liquid molecule

Question 18

If substance X has stronger intermolecular attractions than substance Y,which of the following is most apt to be false?

A)Y has the lower boiling point and higher vapor pressure
B)Y has the higher vapor pressure and lower molar heat of vaporization
C)Y has the higher boiling point and higher molar heat of vaporization
D)X has the higher boiling point and higher molar heat of vaporization
E)X has the lower vapor pressure and higher molar heat of vaporization

Question 19

The structural formula for glycerin is shown below.Compare the intermolecular forces in glycerin with those in n-hexane,C₆H₁₄,in which all carbons are in a continuous chain.Which of the following statements is true?

A)The principal intermolecular forces in glycerin are induced dipole forces; in hexane, hydrogen bonds
B)Hydrogen bonding is present in glycerin, but not in hexane
C)Hydrogen bonding is present in both compounds
D)Both compounds exhibit dipole-dipole forces
E)Induced dipole forces are present in neither compound

Question 20

The kinetic molecular theory as applied to liquids differs in two major ways from the theory as applied to gases.One of these is that:

A)Matter no longer appears to be made up of discrete particles
B)Energy changes result from intermolecular collisions
C)Attractive forces between molecules are significant
D)Molecules are no longer in motion relative to each other
E)Forces between molecules are no longer electrostatic in character

Question 21

A sample of solid silver releases 476 J of heat when cooled from 98.3°C to 21.2°C.The specific heat of silver is 0.24 J/g • °C.What is the mass of the sample?

A)8.8 × 10³ g
B)1.5 × 10⁵ g
C)0.039 g
D)1.5 g
E)25.7 g

Question 22

Calculate the heat of fusion of an unknown pure substance if 5.33 × 10³ kJ of heat is required to melt a 17.2 kg sample.

A)1.09 × 10^-5 J/g
B)3.23 × 10^-3 J/g
C)3.10 × 10² J/g
D)9.17 × 10⁴ J/g
E)3.10 × 10⁵ J/g

Question 23

Consider the following image. What type of solid is represented by this particulate-level model?

A)amorphous solid
B)molecular crystal
C)ionic crystal
D)covalent network solid
E)metallic crystal

Question 24

Among the following,identify the correct statement about a boiling liquid:

A)The temperature of a liquid boiling in an open beaker is equal to the temperature of the gas space above the liquid
B)Equilibrium vapor pressure at the boiling temperature is higher than the surrounding pressure
C)Vapor pressure in a bubble in the liquid is equal to or slightly greater than the equilibrium pressure at boiling temperature
D)Boiling temperature can be increased by boiling in a vacuum
E)All statements are incorrect

Question 25

A substance that melts at 122°C is probably:

A)A network solid
B)An ionic crystal
C)A metallic crystal
D)A molecular crystal
E)A good electrical conductor

Question 26

The main reason equilibrium vapor pressure is greater at higher temperatures is that...

A)A larger fraction of the molecules in the sample has sufficient kinetic energy to move from the liquid phase to the vapor phase
B)The average kinetic energy is greater
C)Intermolecular attractions are weaker
D)The particles are moving at higher speeds
E)The escape energy is decreased

Question 27

The heat of fusion of gold is 63 joules per gram.Once a 25.0 g sample of gold has been heated to its melting point,1063°C,how much additional heat is required to melt it?

A)89 kJ
B)39 kJ
C)2.7 kJ
D)2.6 kJ
E)1.6 kJ

Question 28

The specific heat of solid gold is 0.13 J/g • °C.How much heat is needed to raise the temperature of 25.0 g of gold from 23°C to its melting point at 1063°C?

A)3.5 kJ
B)3.4 kJ
C)0.14 kJ
D)2.0 × 10³ kJ
E)3.3 kJ

Question 29

Why does ice float on liquid water?

A)It is a compound without carbon atoms that exists in the liquid state at room temperature and pressure.
B)The linear structure of the water molecule allows ice molecules to pack together tightly enough to allow ice to float.
C)Ice is structurally similar to wood, so ice floats on water in a manner similar to wooden ships where air becomes trapped in cells within the solid structure.
D)Oxygen's low electronegativity leads to the collapse of the crystal structure, allowing the molecules to become closer together in water.
E)Water molecules in the solid form are held in a crystal pattern that has voids between the molecules.

Question 30

Which of the following statements is correct?

A)There is long-range order in a crystalline solid
B)Graphite is an example of an amorphous solid.
C)Glass, rubber, and plastic are examples of crystalline solids
D)Particles in an amorphous solids are arranged in a distinct geometric order
E)In a crystalline solid particles can move past the closest neighboring particles.

Question 31

How are network solids,such as diamond,C,and quartz,SiO₂,distinguished from molecular crystals such as I₂?

A)Network solids have very high melting points
B)Network solids are ionic, while molecular ones are covalent substances
C)Network solids dissolve in water; molecular ones do not
D)Network solids are excellent conductors of electricity, while molecular crystals are nonconductors
E)Network solids have individual molecules of fixed size; molecular crystals do not

Question 32

Which of the following statements about change of state is false?

A)The boiling point of a liquid depends on the gas pressure above the liquid
B)Condensation is an endothermic process
C)Evaporation occurs at the surface of a liquid, but boiling may occur at any point within the liquid
D)Energy is absorbed by a liquid as it boils
E)A liquid boils when its vapor pressure is slightly greater than the pressure above it

Question 33

The graph below represents a temperature versus energy plot for a pure substance. Identify the point(s)where:
(i)only gas exists
(ii)both solid and liquid exist

A)(i) 7 (ii) 2 and 3
B)(i) 7 (ii) 5 and 6
C)(i) 1 (ii) 2 and 3
D)(i) 4 (ii) 5 and 6
E)(i) 4 (ii) 2 and 3

Question 34

A sample of lead releases 221 kJ of heat when freezing.What is the mass of the sample?
H_fus = 23 J/g

A)9.6 g
B)9.6 × 10³ g
C)5.1 × 10⁶ g
D)2.0 × 10^-7 g
E)1.0 × 10^-4 g

Question 35

Among the following,identify the incorrect statement about a boiling liquid:

A)Boiling temperature may be increased by raising surrounding pressure
B)The temperature of the liquid must be greater than that of the gas above the liquid
C)Boiling in an open beaker occurs at a lower temperature at higher altitudes
D)Equilibrium vapor pressure at boiling temperature equals, or is slightly higher than surrounding pressure
E)All statements are correct

Question 36

What quantity of water will form by the condensation of steam when 276 kJ of heat are removed?
H_vap = 2.26 kJ/g

A)122 g
B)67.8 g
C)2.65 g
D)624 g
E)18.0 g

Question 37

Calculate the specific heat of an unknown metal if a 123 gram sample requires 8.8 kJ of heat to change from 16°C to 97°C.

A)0.88 J/g • °C
B)1.1 J/g • °C
C)5.8 × 10³ J/g • °C
D)1.3 × 10⁴ J/g • °C
E)8.8 × 10⁷ J/g • °C

Question 38

Closed system A consists of liquid acetone in equilibrium with its own vapor at 30°C.System B is like System A,except that the volume of liquid,the area of the liquid surface,and the volume of the vapor space above the liquid are all twice as large as System A,and the temperature is only 15°C.Identify the statement among the following that is positively false.

A)Evaporation and condensation rates are equal in A
B)Evaporation and condensation rates are equal in B
C)Evaporation rate in A is greater than evaporation rate in B
D)Vapor pressure in B is greater than vapor pressure in A
E)Condensation rate in A is greater than condensation rate in B

Question 39

Calculate the heat of vaporization of zinc if 393 kJ is required to vaporize a 223-gram sample.

A)1.14 × 10^-5 kJ/g
B)8.76 × 10⁴ kJ/g
C)0.567 kJ/g
D)1.76 kJ/g
E)2.26 kJ/g

Question 40

Among the following,identify the sentence that states a fact about equilibrium vapor pressure,followed by an acceptable explanation or reason for the fact.

A)Vapor pressure decreases with temperature because the liquid expands and molecules are farther apart
B)Vapor pressure increases with temperature because intermolecular attractions are weaker at higher temperatures
C)Vapor pressure decreases with temperature because molecules stick together better when they are hot
D)Vapor pressure increases with temperature because energy is distributed more efficiently at higher temperatures
E)Vapor pressure increases with temperature because at higher temperatures a larger fraction of the molecules has sufficient energy to escape from the liquid state

Question 41

The graph below represents a temperature versus energy plot for a pure substance.Identify the point(s)...(i)where only liquid exists and (ii)is associated with the heat of vaporization

A)(i) 7 (ii) 2 and 3
B)(i) 7 (ii) 5 and 6
C)(i) 4 (ii) 2 and 3
D)(i) 4 (ii) 5 and 6
E)(i) 1 (ii) 5 and 6

Question 42

What is the total heat flow if 18 grams of water at 12°C is heated to become steam at 109°C? The specific heat of liquid water is 4.18 J/g • 0°C; the specific heat of steam is 2.0 J/g • 0°C.The heat of vaporization of water is 2.26 kJ/g,and the boiling point of water is 100°C.

A)0.32 kJ
B)6.6 kJ
C)48 kJ
D)41 kJ
E)7.0 × 10³ kJ

Question 43

The graph below represents a temperature versus energy plot for a pure substance. Identify the point(s) (i)where both liquid and gas exist and (ii)is associated with the heat of condensation

A)(i) 1 (ii) 5 and 6
B)(i) 2 and 3 (ii) 5 and 6
C)(i) 4 (ii) 5 and 6
D)(i) 5 and 6 (ii) 5 and 6
E)(i) 7 (ii) 3 and 3

Question 44

What is the total heat flow if 27 grams of steam at 143°C is cooled to become water at 34°C? The specific heat of water is 4.18 J/g • °C; the specific heat of steam is 2.0 J/g • °C.The heat of vaporization of water is 2.26 kJ/g,and the boiling point of water is 100°C.

A)2.3 kJ
B)7.4 kJ
C)61 kJ
D)71 kJ
E)9.8 × 10³ kJ

Question 45

What is the total heat flow if 28 grams of water at 12°C is cooled to become ice at -19°C? The specific heat of liquid water is 4.18 J/g • °C; the specific heat of ice is 2.1 J/g • °C.The heat of fusion of ice is 333 J/g,and the freezing point of water is 0.0°C.

A)1.1 kJ
B)1.4 kJ
C)9.4 kJ
D)10.8 kJ
E)11.8 kJ