Question 1

Which of the following statements is correct?

Accepted Answer

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. 
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 2

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

Accepted Answer

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

Question 3

If there were no intermolecular forces, most matter would be in the gas phase at room temperature.

Accepted Answer

A) True 
 B)False

Question 4

Which of the following has the highest boiling point?

Accepted Answer

A) H2 
B) HF 
C) HCl 
D) HBr 
E) HI 
A) H2 
B) HF 
C) HCl 
D) HBr 
E) HI

Question 5

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

Accepted Answer

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

Question 6

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 7

What causes water to have a high boiling point, high viscosity, and high surface tension, compared to other liquids?

Accepted Answer

Water has a high boiling point, high vis

Question 8

Which of the following molecules experience dipole-dipole forces?

Accepted Answer

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

Question 9

Which of the following statements is correct?

Accepted Answer

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. 
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

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

Accepted Answer

A) F2 2 
B) F2 2 
C) F2 2 2 2 
E) Cl2 2 < Ne < He 
A) F2 2 
B) F2 2 
C) F2 2 2 2 
E) Cl2 2 < Ne < He

Question 11

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

Question 12

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

Accepted Answer

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

Question 13

Calculate the amount of heat energy in kJ required to convert 24.0 g of water at 25.5°C to steam at 124.0°C. (Cwater = 4.18 J/g°C; Csteam = 2.02 J/g°C; molar heat of vaporization of liquid water = 4.07 × 104 J/mol)

Accepted Answer

To calculate the amount of heat energy r

Question 14

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)

Accepted Answer

A) 4.50 × 102 kJ 
B) 25.0 kJ 
C) 13.0 kJ 
D) 2.25 × 103 kJ 
E) 4.50 × 10−1 kJ 
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 15

Explain why different liquids have different vapor pressures at a given temperature by filling in the blanks in the following statements: Different liquids have differing amounts of ________. Liquids with ________ intermolecular forces vaporize more easily at a given temperature, and thus will have a ________ vapor pressure than a liquid with ________ intermolecular forces.

Accepted Answer

Different liquids have differing amounts

Question 16

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?

Accepted Answer

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

Question 17

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

Accepted Answer

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

Question 18

Which substance has the highest melting point?

Accepted Answer

A) Br2 
B) C6H10 
C) Ar 
D) KBr 
E) Cl2 
A) Br2 
B) C6H10 
C) Ar 
D) KBr 
E) Cl2

Which of the following statements is correct?

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

If there were no intermolecular forces, most matter would be in the gas phase at room temperature.

Which of the following has the highest boiling point?

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

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.

What causes water to have a high boiling point, high viscosity, and high surface tension, compared to other liquids?

Which of the following molecules experience dipole-dipole forces?

Which of the following statements is correct?

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

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

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

Calculate the amount of heat energy in kJ required to convert 24.0 g of water at 25.5°C to steam at 124.0°C. (C_water = 4.18 J/g°C; C_steam = 2.02 J/g°C; molar heat of vaporization of liquid water = 4.07 × 10⁴ J/mol)

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)

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?

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

Which substance has the highest melting point?

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

Which of the following statements is correct?

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

If there were no intermolecular forces, most matter would be in the gas phase at room temperature.

Which of the following has the highest boiling point?

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

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.

What causes water to have a high boiling point, high viscosity, and high surface tension, compared to other liquids?

Which of the following molecules experience dipole-dipole forces?

Which of the following statements is correct?

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

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

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

Calculate the amount of heat energy in kJ required to convert 24.0 g of water at 25.5°C to steam at 124.0°C. (Cwater = 4.18 J/g°C; Csteam = 2.02 J/g°C; molar heat of vaporization of liquid water = 4.07 × 104 J/mol)

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)

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?

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

Which substance has the highest melting point?

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

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

Calculate the amount of heat energy in kJ required to convert 24.0 g of water at 25.5°C to steam at 124.0°C. (C_water = 4.18 J/g°C; C_steam = 2.02 J/g°C; molar heat of vaporization of liquid water = 4.07 × 10⁴ J/mol)

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)