Exam 10: The Liquid and Solid States

Calculate the amount of heat energy in kJ required to convert 45.0 g of ice at -15.5°C to steam at 124.0°C. (C_water = 4.18 J/g°C; C_ice = 2.03 J/g°C; 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)

(Short Answer)

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Question 21

Which choice correctly lists the intermolecular forces present in CH₃Br?

(Multiple Choice)

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Question 22

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?

(Multiple Choice)

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Question 23

Which substance has the highest melting point?

(Multiple Choice)

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Question 24

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

(Multiple Choice)

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Question 25

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

(Multiple Choice)

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Question 26

Which of the following statements regarding intermolecular forces is incorrect?

(Multiple Choice)

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Question 27

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

(Multiple Choice)

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Question 28

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

(Multiple Choice)

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Question 29

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

(Multiple Choice)

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Question 30

CH₃OH boils at 64.7°C, and C₂H₆ boils at -88°C. Which types of intermolecular forces are responsible for the difference in their boiling points?

(Short Answer)

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Question 31

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

(Multiple Choice)

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Question 32

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

(Multiple Choice)

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Question 33

One would expect that since CO is polar, it has a higher boiling point than C₆H₁₄.

(True/False)

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Question 34

Which of the following statements is correct?

(Multiple Choice)

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Question 35

(True/False)

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Question 36

Consider the melting point of the following solids. Which of these solids is most likely a molecular solid?

(Multiple Choice)

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Question 37

The molecular-level diagram of the substance shown must represent a liquid, since the atoms are not very close to one another.

(True/False)

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Question 38

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.)

(Multiple Choice)

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Question 39

(Multiple Choice)

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Question 40

Showing 21 - 40 of 118

Calculate the amount of heat energy in kJ required to convert 45.0 g of ice at -15.5°C to steam at 124.0°C. (C_water = 4.18 J/g°C; C_ice = 2.03 J/g°C; 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)

Which choice correctly lists the intermolecular forces present in CH₃Br?

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?

Which substance has the highest melting point?

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

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

Which of the following statements regarding intermolecular forces is incorrect?

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

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

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

CH₃OH boils at 64.7°C, and C₂H₆ boils at -88°C. Which types of intermolecular forces are responsible for the difference in their boiling points?

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

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

One would expect that since CO is polar, it has a higher boiling point than C₆H₁₄.

Which of the following statements is correct?

The substance shown in the figure must be a solid because you cannot see through it. ©Jim Birk

Consider the melting point of the following solids. Which of these solids is most likely a molecular solid?

The molecular-level diagram of the substance shown must represent a liquid, since the atoms are not very close to one another.

Identify the type of solid shown in the image. © C Squared Studios/Getty Images

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Exam 10: The Liquid and Solid States

Calculate the amount of heat energy in kJ required to convert 45.0 g of ice at -15.5°C to steam at 124.0°C. (Cwater = 4.18 J/g°C; Cice = 2.03 J/g°C; Csteam = 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)

Which choice correctly lists the intermolecular forces present in CH3Br?

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?

Which substance has the highest melting point?

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

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

Which of the following statements regarding intermolecular forces is incorrect?

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

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

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

CH3OH boils at 64.7°C, and C2H6 boils at -88°C. Which types of intermolecular forces are responsible for the difference in their boiling points?

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

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

One would expect that since CO is polar, it has a higher boiling point than C6H14.

Which of the following statements is correct?

The substance shown in the figure must be a solid because you cannot see through it. ©Jim Birk

Consider the melting point of the following solids. Which of these solids is most likely a molecular solid?

The molecular-level diagram of the substance shown must represent a liquid, since the atoms are not very close to one another.

Identify the type of solid shown in the image. © C Squared Studios/Getty Images

Matter and Energy

Atoms, Ions, and the Periodic Table

Chemical Compounds

Chemical Composition

Chemical Reactions and Equations

Quantities in Chemical Reactions

Electron Structure of the Atom

Chemical Bonding

The Gaseous State

Solutions

Reaction Rates and Chemical Equilibrium

Acids and Bases

Oxidation-Reduction Reactions

Nuclear Chemistry

Organic Chemistry

Biochemistry

Filters

Calculate the amount of heat energy in kJ required to convert 45.0 g of ice at -15.5°C to steam at 124.0°C. (C_water = 4.18 J/g°C; C_ice = 2.03 J/g°C; 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)

Which choice correctly lists the intermolecular forces present in CH₃Br?

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

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

CH₃OH boils at 64.7°C, and C₂H₆ boils at -88°C. Which types of intermolecular forces are responsible for the difference in their boiling points?

One would expect that since CO is polar, it has a higher boiling point than C₆H₁₄.