Question 1

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

Accepted Answer

A) 4.50 x 102 kJ 
B) 25.0 kJ 
C) 13.0 kJ 
D) 2.25 x 103 kJ 
E) 4.50 x 10-1 kJ 
A) 4.50 x 102 kJ 
B) 25.0 kJ 
C) 13.0 kJ 
D) 2.25 x 103 kJ 
E) 4.50 x 10-1 kJ

Question 2

Detergents are used to increase the surface tension of water, so that it will stay in the shape of a droplet.

Accepted Answer

A) True 
 B)False

Question 3

The molecular-level diagram shows the process of evaporation.

Accepted Answer

A) True 
 B)False

Question 4

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

Accepted Answer

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

Question 5

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

Accepted Answer

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

Question 6

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

Accepted Answer

A) I2  
B) Pb 
C) Ar 
D) CCl4  
E) C8H18  
A) I2  
B) Pb 
C) Ar 
D) CCl4  
E) C8H18

Question 7

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

Accepted Answer

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

Question 8

Which choice correctly lists the intermolecular forces present in CH3Br?

Accepted Answer

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 
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 9

Which of the following has the strongest London dispersion forces?

Accepted Answer

A) CH4  
B) CF4  
C) CCl4  
D) CBr4  
E) CI4  
A) CH4  
B) CF4  
C) CCl4  
D) CBr4  
E) CI4

Question 10

A solid substance has a very low melting point, is soft, and does not conduct heat or electricity.This substance is probably a(n)________ solid.

Accepted Answer

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

Question 11

Which of the following statements regarding intermolecular forces is incorrect?

Accepted Answer

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. 
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 12

Calculate the amount of heat energy required to evaporate 27.5 g of water at 100.0 $\degree$C.(molar heat of vaporization of liquid water = 4.07 x 104 J/mol)

Accepted Answer

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

Question 13

Of the two molecules shown in the figure, one would expect that CO2 has a higher boiling point than NO2 because CO2 is linear and nonpolar.

Accepted Answer

A) True 
 B)False

Question 14

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

Accepted Answer

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. 
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 15

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

Accepted Answer

A) CBr4  
B) F2  
C) Mn 
D) C6H14  
E) Sr 
A) CBr4  
B) F2  
C) Mn 
D) C6H14  
E) Sr

Question 16

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

Accepted Answer

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

Question 17

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

Accepted Answer

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

Question 18

Which choice correctly lists the intermolecular forces present in CH4?

Accepted Answer

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 
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 19

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

Accepted Answer

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 
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

Question 20

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

Accepted Answer

A) Cl2 2  
B) Ar 2 2  
C) Ne 2 2  
D) Ne 2 2  
E) Cl2 2 < Ar < Ne 
A) Cl2 2  
B) Ar 2 2  
C) Ne 2 2  
D) Ne 2 2  
E) Cl2 2 < Ar < Ne

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

Detergents are used to increase the surface tension of water, so that it will stay in the shape of a droplet.

The molecular-level diagram shows the process of evaporation.

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

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

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

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

Which choice correctly lists the intermolecular forces present in CH₃Br?

Which of the following has the strongest London dispersion forces?

A solid substance has a very low melting point, is soft, and does not conduct heat or electricity.This substance is probably a(n)________ solid.

Which of the following statements regarding intermolecular forces is incorrect?

Calculate the amount of heat energy required to evaporate 27.5 g of water at 100.0 $\degree$ C.(molar heat of vaporization of liquid water = 4.07 x 10⁴ J/mol)

Of the two molecules shown in the figure, one would expect that CO₂ has a higher boiling point than NO₂ because CO₂ is linear and nonpolar.

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

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

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

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

Which choice correctly lists the intermolecular forces present in CH₄?

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

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

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

Exam 10: The Liquid and Solid States

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

Detergents are used to increase the surface tension of water, so that it will stay in the shape of a droplet.

The molecular-level diagram shows the process of evaporation.

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

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

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

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

Which choice correctly lists the intermolecular forces present in CH3Br?

Which of the following has the strongest London dispersion forces?

A solid substance has a very low melting point, is soft, and does not conduct heat or electricity.This substance is probably a(n)________ solid.

Which of the following statements regarding intermolecular forces is incorrect?

Calculate the amount of heat energy required to evaporate 27.5 g of water at 100.0 °\degree° C.(molar heat of vaporization of liquid water = 4.07 x 104 J/mol)

Of the two molecules shown in the figure, one would expect that CO2 has a higher boiling point than NO2 because CO2 is linear and nonpolar.

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

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

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

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

Which choice correctly lists the intermolecular forces present in CH4?

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

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

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 units of kilojoules, required to melt 75.0 g of ice at 0.0 $\degree$ C.(molar heat of fusion of ice = 6.01 x 10³ J/mol)

Which choice correctly lists the intermolecular forces present in CH₃Br?

Calculate the amount of heat energy required to evaporate 27.5 g of water at 100.0 $\degree$ C.(molar heat of vaporization of liquid water = 4.07 x 10⁴ J/mol)

Of the two molecules shown in the figure, one would expect that CO₂ has a higher boiling point than NO₂ because CO₂ is linear and nonpolar.

Which choice correctly lists the intermolecular forces present in CH₄?

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