Deck 7: Solids, Liquids, and Phase Changes

Question 1

Which has the highest surface tension at room temperature?

A)CH₄
B)CF₄
C)CCl₄
D)CBr₄
E)CI₄

Answer 1

CI₄

Question 2

Ammonia's unusually high melting point is the result of

A)dipole-dipole forces.
B)London dispersion forces.
C)hydrogen bonding.
D)covalent bonding.
E)ionic bonding.

Answer 2

hydrogen bonding.

Question 3

Place the substances in order of increasing melting point. CS₂ KCl NF₃

A)CS₂ < NF₃ < KCl
B)KCl < NF₃ < CS₂
C)NF₃ < CS₂ < KCl
D)CS₂ < KCl < NF₃
E)NF₃ < KCl < CS₂

Answer 3

CS₂ < NF₃ < KCl

Question 4

What is determined by the magnitude of intermolecular forces in a liquid and is a measure of a fluid's resistance to flow?

A)Surface tension
B)Adhesion
C)Polarity
D)Viscosity
E)Cohesion

Question 5

Which one of the following crystallizes in a metallic lattice?

A)C
B)NaMnO₄
C)K
D)LiClO₄
E)K₂Cr₂O₇

Question 6

Place the substances in order of increasing viscosity. CH₃OH C₂H₆ HO-CH₂CH₂-OH

A)C₂H₆ < HO-CH₂CH₂-OH < CH₃OH
B)CH₃OH< C₂H₆ < HO-CH₂CH₂-OH
C)HO-CH₂CH₂-OH< C₂H₆ < CH₃OH
D)CH₃OH < HO-CH₂CH₂-OH < C₂H₆
E)C₂H₆ < CH₃OH < HO-CH₂CH₂-OH

Question 7

For the solid forms of the following elements, which one is most likely to be of the molecular type?

A)Cs
B)C
C)Pb
D)S
E)Cr

Question 8

Which state of matter is described as having a definite shape and volume?

A)solid
B)liquid
C)gas
D)solution
E)mixture

Question 9

Which of the substances would form an ionic solid?

A)NCl₃
B)NH₄Cl
C)Ag
D)He
E)OF₂

Question 10

The energy required to increase the surface of a liquid per unit area is called the

A)capillary action.
B)surface tension.
C)viscosity.
D)cohesion.
E)specific elasticity.

Question 11

Which of the following lacks a regular three-dimensional arrangement of atoms?

A)crystalline solids
B)ionic crystals
C)solids
D)amorphous solids
E)molecular solids

Question 12

If liquid bromine is cooled to form a solid, which type of solid does it form?

A)atomic
B)metallic
C)molecular
D)ionic
E)covalent

Question 13

Which state of matter is described as taking on the shape and volume of its container?

A)solid
B)liquid
C)gas
D)solution
E)mixture

Question 14

Which state of matter is described as taking on the shape of its container, but having a specific volume?

A)solid
B)liquid
C)gas
D)solution
E)mixture

Question 15

Place the substances in order of increasing melting point. CO₂ CH₄ OF₂

A)OF₂ < CO₂ < CH₄
B)CH₄ < CO₂ < OF₂
C)OF₂ < CH₄ < CO₂
D)CO₂ < CH₄ < OF₂
E)CO₂ < OF₂ < CH₄

Question 16

Which of the following statements is ?

A)The higher the viscosity, the faster a liquid flows.
B)The viscosity increases with increasing temperature.
C)The stronger the intermolecular forces, the higher the viscosity.
D)Hydrogen bonding in water gives rise to its unusually low viscosity.
E)The viscosity of gases is larger than the viscosity of liquids.

Question 17

Ethanol (C₂H₅-OH) will have a greater viscosity than ethylene glycol (HO-CH₂CH₂-OH) at the same temperature.

Question 18

Which of the substances would form a metallic solid?

A)NCl₃
B)KCl
C)Ni
D)Ar
E)MgF₂

Question 19

Place the substances in order of increasing melting point. CH₄
C₃H₈
C₂H₄

A)C₃H₈ < C₂H₄ < CH₄
B)C₂H₄ < CH₄ < C₃H₈
C)C₃H₈ < CH₄ < C₂H₄
D)CH₄ < C₂H₄ < C₃H₈
E)C₂H₄ < C₃H₈ < CH₄

Question 20

Which of the following terms refers to the resistance of a liquid to flow?

A)Surface tension
B)Capillary action
C)Viscosity
D)Adhesion
E)Cohesion

Question 21

What is the process in which molecules undergo a phase change from the gas phase to the liquid phase?

A)vaporization
B)condensation
C)freezing
D)melting
E)sublimation

Question 22

What is the process in which molecules undergo a phase change from the solid phase to the liquid phase?

A)vaporization
B)condensation
C)freezing
D)melting
E)sublimation

Question 23

Place the substances in order of decreasing boiling point. BeCl₂ CBr₄ BeBr₂

A)BeCl₂ > CBr₄ > BeBr₂
B)BeCl₂ > BeBr₂ > CBr₄
C)CBr₄ > BeBr₂ > BeCl₂
D)BeBr₂ > BeCl₂ > CBr₄

Question 24

What is q if 28.6 g of water is heated from 22.0°C to 78.3°C? The specific heat of water is 4.184 J/g·°C.

A)2.60 J
B)2.63 kJ
C)6.74 kJ
D)9.37 kJ
E)3.94×10⁴ kJ

Question 25

What is the process in which molecules undergo a phase change from the liquid phase to the gas phase?

A)vaporization
B)condensation
C)freezing
D)melting
E)sublimation

Question 26

The specific heat (capacity) is

A)amount of energy needed to change 1 g of a substance by 1°C.
B)amount of energy needed to change 1 mol of a substance by 1°C
C)amount of energy required to melt 1 g of substance.
D)amount of substance that is heated by 1°C.
E)the temperature increase, in K, associated with heating 1 g of a substance for 1 minute.

Question 27

Which of the following properties indicates the presence of strong intermolecular forces in a liquid?

A)a low heat of vaporization
B)a low critical temperature
C)a low vapor pressure
D)a low boiling point
E)a low melting point

Question 28

Which corresponds to the temperature-dependent partial pressure above the surface of a liquid?

A)Surface tension
B)Vapor pressure
C)Boiling point
D)Viscosity
E)Capillary action

Question 29

Which substance has the highest vapor pressure at room temperature?

A)HF
B)HCl
C)HBr
D)HI
E)All of these substances have the same vapor pressure at room temperature.

Question 30

What is the process in which molecules undergo a phase change from the liquid phase to the solid phase?

A)vaporization
B)condensation
C)freezing
D)melting
E)sublimation

Question 31

Select the pair of substances in which the one with the lower vapor pressure at a given temperature is listed first.

A)
B)PH₃, NH₃
C) CF₄, CBr₄
D)C₃H₈,C₄H₁₀
E)F₂, Cl₂

Question 32

Which statement concerning the vapor pressures of water and methanol (CH₃OH) is ?

A)At 25ºC, methanol has a higher vapor pressure than water because methanol has a lower normal boiling point than water.
B)At 25ºC, methanol has a higher vapor pressure than water because methanol is a poorer solvent than water.
C)At 25ºC, methanol has a higher vapor pressure than water because methanol is a less viscous liquid than water.
D)At 25ºC, methanol has a higher vapor pressure than water because the density of methanol is less than the density of water.
E)At 25ºC, methanol has a higher vapor pressure than water because methanol has weaker intermolecular forces than water.

Question 33

Place the substances in order of decreasing boiling point. CO₂ CH₄ OF₂

A)OF₂ > CO₂ > CH₄
B)CH₄ > CO₂ > OF₂
C)OF₂ > CH₄ > CO₂
D)CO₂ > CH₄ > OF₂
E)CO₂ > OF₂ > CH₄

Question 34

What is the process in which molecules undergo a phase change directly from the gas phase to the solid phase?

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

Question 35

Which substance has the lowest vapor pressure at room temperature?

A)HF
B)HCl
C)HBr
D)HI
E)H₂

Question 36

Place the substances in order of increasing viscosity. CH₃CH₂CH₂CH₃ H₂NCH₂CH₂NH₂ CH₃CH₂CH₂NH₂

A)CH₃CH₂CH₂CH₃ < CH₃CH₂CH₂NH₂ < H₂NCH₂CH₂NH₂
B)H₂NCH₂CH₂NH₂ < CH₃CH₂CH₂NH₂ < CH₃CH₂CH₂CH₃
C)H₂NCH₂CH₂NH₂ < CH₃CH₂CH₂CH₃ < CH₃CH₂CH₂NH₂
D)CH₃CH₂CH₂CH₃ < H₂NCH₂CH₂NH₂ < CH₃CH₂CH₂NH₂
E)CH₃CH₂CH₂NH₂ < H₂NCH₂CH₂NH₂ < CH₃CH₂CH₂CH₃

Question 37

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

A)C₇H₁₆, C₅H₁₂
B)CCl₄, CBr₄
C)H₂O, H₂S
D)CH₃CH₂OH, CH₃-O-CH₃
E)Xe, Kr

Question 38

Place the substances in order of increasing boiling point. BF₃ NF₃ BeF₂

A)NF₃ < BF₃ < BeF₂
B)BF₃ < NF₃ < BeF₂
C)NF₃ < BeF₂ < BF₃
D)BeF₂ < NF₃ < BF₃
E)BeF₂ < BF₃ < NF₃

Question 39

Place the substances in order of increasing boiling point. BeF₂ SF₂ Ar

A)BeF₂ < SF₂ < Ar
B)Ar < BeF₂ < SF₂
C)SF₂ < Ar < BeF₂
D)SF₂ < BeF₂ < Ar
E)Ar < SF₂ < BeF₂

Question 40

What is the process in which molecules undergo a phase change directly from the solid phase to the gas phase?

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

Question 41

How much heat is required to raise the temperature of 1500 g of water from 25°C to 52°C? The specific heat of water is 4.184 J/g·°C.

A)1500 kJ
B)170 kJ
C)6.3 kJ
D)41 J
E)41 kJ

Question 42

When Karl Kaveman adds chilled grog to his new granite mug, he removes 10.9 kJ of energy from the mug.If it has a mass of 625 g and was at 25°C, what is its new temperature? Specific heat capacity of granite = 0.79 J/g·°C.

A)3°C
B)14°C
C)22°C
D)47°C
E)None of these choices is correct.

Question 43

Benzene is a starting material in the synthesis of nylon fibers and polystyrene (styrofoam).Its specific heat capacity is 1.74 J/g·°C.If 16.7 kJ of energy is absorbed by a 225-g sample of benzene at 20.0°C, what is its final temperature?

A)−22.7°C
B)37.7°C
C)42.7°C
D)62.7°C
E)80.1°C

Question 44

Ethylene glycol, used as a coolant in automotive engines, has a specific heat capacity of 2.42 J/g·°C.Calculate q when 3.65 kg of ethylene glycol is cooled from 132°C to 85°C.

A)−1900 kJ
B)−420 kJ
C)−99 kJ
D)−0.42 kJ
E)−4.2 × 10⁻⁶ kJ

Question 45

What is the energy in kJ/mol required to melt 1 mole of a solid?

A)molar heat of freezing
B)molar heat of fission
C)molar heat of vaporization
D)molar heat of fusion
E)molar heat of condensation

Question 46

If 325 g of water at 4.2°C absorbs 12.28 kJ, what is the final temperature of the water? The specific heat of water is 4.184 J/g·°C.

A)4.21°C
B)4.8°C
C)9.0°C
D)13.2°C
E)2938°C

Question 47

What mass of water would need to evaporate from your skin in order to dissipate 1.70 ×10⁵ J of heat from the surface of your body? H₂O(l) → H₂O(g) ∆H_vap = 40.7 kJ/mol

A)2.26 g
B)4.18 g
C)75.2 g
D)4.18 ×10³ g
E)4.07 × 10⁴ g

Question 48

What amount of energy (heat) is required to warm a 73.5-g sample of liquid ethanol from 15.0ºC to 29.5ºC? The specific heat capacity of ethanol is 2.46 J/gºC.

A)0.485 J
B)433 J
C)2.62 × 10³ J
D)5.33 × 10³ J
E)238 J

Question 49

If, as a pioneer, you wished to warm your room by taking an object heated on top of a pot-bellied stove to it, which of the following 15-pound objects, each heated to 100°C, would be the best choice? The specific heat capacity (in J/g·°C) for each substance is given in parentheses.Iron (0.450), copper (0.387), granite (0.79), gold (0.129), water (4.184).

A)iron
B)copper
C)granite
D)gold
E)H₂O

Question 50

A piece of copper with a mass of 218 g has a heat capacity of 83.9 J/°C.What is the specific heat of copper?

A)0.385 J/g·°C
B)1.83 × 10⁴ J/g·°C
C)2.60 J/g·°C
D)1.32 J/g·°C
E)24.5 J/g·°C

Question 51

What quantity of heat is required to melt 2.00 kg of iron at its melting point (1809 K)? For iron, ∆H_fus = 13.80 kJ/mol.

A)0.385 kJ
B)6.90 kJ
C)27.6 kJ
D)494 kJ
E)771 kJ

Question 52

A 275-g sample of nickel at l00.0°C is placed in 100.0 g of water at 22.0°C.What is the final temperature of the water? Assume no heat transfer with the surroundings.The specific heat of nickel is 0.444 J/g·°C and the specific heat of water is 4.184 J/g·°C.

A)39.6°C
B)40.8°C
C)61.0°C
D)79.2°C
E)82.4°C

Question 53

How much heat is required to raise the temperature of 22.8 g of copper from 20.0°C to 875.0°C? The specific heat of copper is 0.385 J/g·°C.

A)14.4 J
B)176 J
C)7.51 kJ
D)7.68 kJ
E)9.90 kJ

Question 54

What is the change in temperature if a 25.0-g block of aluminum absorbs 10.0 kJ of heat? The specific heat of aluminum is 0.900 J/g·°C.

A)0.44°C
B)22.5°C
C)225°C
D)360°C
E)444°C

Question 55

How much heat is required to raise the temperature of 12.0 g of water from 15.4°C to 93.0°C? The specific heat of water is 4.184 J/g·°C.

A)223 J
B)773 J
C)503 J
D)4.67 ×10³ J
E)3.90 ×10³ J

Question 56

If 75.4 J of energy is absorbed by 0.25 mol of CCl₄ at constant pressure, what is the change in temperature? The specific heat of CCl₄ is 0.861 J/g·°C.

A)17.8°C
B)21.9°C
C)2.3°C
D)9.1°C
E)44.6°C

Question 57

A glass containing 200.0 g of H₂O at 20.0°C was placed in a refrigerator.The water loses 11.7 kJ as it cools to a constant temperature.What is its new temperature? The specific heat of water is 4.184 J/g·°C.

A)0.0°C
B)4.0°C
C)6.0°C
D)14.0°C
E)34.0°C

Question 58

What amount of energy (heat) is required to warm a 65.0-g sample of liquid water from 25.0ºC to 96.5ºC? The specific heat capacity of water is 4.184 J/gºC.

A)4.60 J
B)1.11 × 10³ J
C)2.62 × 10⁴ J
D)1.94 ×10⁴ J
E)1.61 J