Question 1

Which substance has the highest melting point?

Accepted Answer

A) Mn 
B) C8H18 
C) Ar 
D) C (diamond) 
E) Br2 
A) Mn 
B) C8H18 
C) Ar 
D) C (diamond) 
E) Br2 D

Question 2

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 C

Question 3

The physical properties of a substance influenced by the strength of intermolecular forces include all of the following except

Accepted Answer

A) melting point. 
B) boiling point. 
C) viscosity. 
D) vapor pressure. 
E) mass. 
A) melting point. 
B) boiling point. 
C) viscosity. 
D) vapor pressure. 
E) mass. E

Question 4

What phase transition is occurring between points B and C on the cooling curve?

Accepted Answer

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

Question 5

Which of the following has the highest boiling point?

Accepted Answer

A) H2 
B) H2O 
C) H2S 
D) H2Se 
E) H2Te 
A) H2 
B) H2O 
C) H2S 
D) H2Se 
E) H2Te

Question 6

Explain how a pressure cooker works by filling in the blanks in the following statement: A pressure cooker allows the pressure inside the cooker to become ________ than atmospheric pressure, which ________ the boiling point of the water used to cook the food, thus cooking the food ________.

Accepted Answer

A pressure cooker allows the pressure in

Question 7

HCl boils at -85°C and F2 boils at -188°C. Which type of intermolecular force is responsible for the higher boiling point of HCl?

Accepted Answer

The higher boiling point of HCl (hydroch

Question 8

Calculate the amount of heat energy required to convert 27.5 g of water at 62.5°C to steam at 124.0°C. (Cwater = 4.184 J/g°C; Cice = 2.03 J/gºC; 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)

Accepted Answer

A) 6.15 × 104 kJ 
B) 1.23 × 102 kJ 
C) 4.31 × 102 kJ 
D) 67.8 kJ 
E) 1.33 kJ 
A) 6.15 × 104 kJ 
B) 1.23 × 102 kJ 
C) 4.31 × 102 kJ 
D) 67.8 kJ 
E) 1.33 kJ

Question 9

Which of the following statements is correct?

Accepted Answer

A) At the melting point of a substance, the solid, liquid, and gas phases are all in equilibrium. 
B) The freezing point and the melting point of a substance are the same. 
C) There is no fundamental difference in the melting process for covalent substances and ionic substances. 
D) In order for a substance to go from the gas phase to the liquid phase, it must absorb energy from the surroundings. 
E) In order for a substance to go from the liquid phase to the gas phase, it must give off energy to the surroundings. 
A) At the melting point of a substance, the solid, liquid, and gas phases are all in equilibrium. 
B) The freezing point and the melting point of a substance are the same. 
C) There is no fundamental difference in the melting process for covalent substances and ionic substances. 
D) In order for a substance to go from the gas phase to the liquid phase, it must absorb energy from the surroundings. 
E) In order for a substance to go from the liquid phase to the gas phase, it must give off energy to the surroundings.

Question 10

The atmospheric pressure on Mount Everest is about 0.30 atm. From the vapor pressure curve of propane, it can be seen the boiling point of propane at this elevation is about ________.

Accepted Answer

A) −137ºC 
B) −120ºC 
C) −67ºC 
D) −42ºC 
E) 0ºC 
A) −137ºC 
B) −120ºC 
C) −67ºC 
D) −42ºC 
E) 0ºC

Question 11

Identify the type of solid shown in the image.

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 12

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, H2S 
B) CH3CH2OH, CH3OH 
C) CH3COCH3, CH3CH2CH2OH 
D) NH3, PH3 
E) Br2, Cl2 
A) H2O, H2S 
B) CH3CH2OH, CH3OH 
C) CH3COCH3, CH3CH2CH2OH 
D) NH3, PH3 
E) Br2, Cl2

Question 13

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 14

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

Accepted Answer

A) Cs 
B) SO2 
C) I2 
D) CCl4 
E) Ni 
A) Cs 
B) SO2 
C) I2 
D) CCl4 
E) Ni

Question 15

The physical properties of a substance influenced by the strength of intermolecular forces include all of the following except

Accepted Answer

A) density. 
B) boiling point. 
C) surface tension. 
D) melting point. 
E) mass. 
A) density. 
B) boiling point. 
C) surface tension. 
D) melting point. 
E) mass.

Question 16

A solid substance has a high melting point, is hard, brittle, and conducts electricity when molten. 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 17

Calculate the amount of heat energy required to evaporate 27.5 g of water at 100.0ºC. (molar heat of vaporization of liquid water = 4.07 × 104 J/mol)

Accepted Answer

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

Question 18

The forces that hold graphite, C(s), together in the solid state are

Accepted Answer

A) ionic bonds. 
B) dipole-dipole forces. 
C) London dispersion forces only. 
D) covalent bonds and London dispersion forces. 
E) attractions between nuclei and delocalized valence electrons. 
A) ionic bonds. 
B) dipole-dipole forces. 
C) London dispersion forces only. 
D) covalent bonds and London dispersion forces. 
E) attractions between nuclei and delocalized valence electrons.

Question 19

Which substance has the highest melting point?

Accepted Answer

A) Mg 
B) C5H12 
C) Kr 
D) SiO2 (silica) 
E) Cl2 
A) Mg 
B) C5H12 
C) Kr 
D) SiO2 (silica) 
E) Cl2

Question 20

What is the boiling point in °C of acetone at 1.2 atm?

Accepted Answer

The answer of What is the boiling point in °C...

Which substance has the highest melting point?

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

The physical properties of a substance influenced by the strength of intermolecular forces include all of the following except

What phase transition is occurring between points B and C on the cooling curve?

Which of the following has the highest boiling point?

Explain how a pressure cooker works by filling in the blanks in the following statement: A pressure cooker allows the pressure inside the cooker to become than atmospheric pressure, which the boiling point of the water used to cook the food, thus cooking the food .

HCl boils at -85°C and F₂ boils at -188°C. Which type of intermolecular force is responsible for the higher boiling point of HCl?

Calculate the amount of heat energy required to convert 27.5 g of water at 62.5°C to steam at 124.0°C. (C_water = 4.184 J/g°C; C_ice = 2.03 J/gºC; 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 of the following statements is correct?

The atmospheric pressure on Mount Everest is about 0.30 atm. From the vapor pressure curve of propane, it can be seen the boiling point of propane at this elevation is about ________.

Identify the type of solid shown in the image.

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

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

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

The physical properties of a substance influenced by the strength of intermolecular forces include all of the following except

A solid substance has a high melting point, is hard, brittle, and conducts electricity when molten. This substance is probably a(n)________ solid.

Calculate the amount of heat energy required to evaporate 27.5 g of water at 100.0ºC. (molar heat of vaporization of liquid water = 4.07 × 10⁴ J/mol)

The forces that hold graphite, C(s), together in the solid state are

Which substance has the highest melting point?

What is the boiling point in °C of acetone at 1.2 atm?

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

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Exam 10: The Liquid and Solid States

Which substance has the highest melting point?

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

The physical properties of a substance influenced by the strength of intermolecular forces include all of the following except

What phase transition is occurring between points B and C on the cooling curve?

Which of the following has the highest boiling point?

Explain how a pressure cooker works by filling in the blanks in the following statement: A pressure cooker allows the pressure inside the cooker to become ________ than atmospheric pressure, which ________ the boiling point of the water used to cook the food, thus cooking the food ________.

HCl boils at -85°C and F2 boils at -188°C. Which type of intermolecular force is responsible for the higher boiling point of HCl?

Calculate the amount of heat energy required to convert 27.5 g of water at 62.5°C to steam at 124.0°C. (Cwater = 4.184 J/g°C; Cice = 2.03 J/gºC; 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 of the following statements is correct?

The atmospheric pressure on Mount Everest is about 0.30 atm. From the vapor pressure curve of propane, it can be seen the boiling point of propane at this elevation is about ________.

Identify the type of solid shown in the image.

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

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

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

The physical properties of a substance influenced by the strength of intermolecular forces include all of the following except

A solid substance has a high melting point, is hard, brittle, and conducts electricity when molten. This substance is probably a(n)________ solid.

Calculate the amount of heat energy required to evaporate 27.5 g of water at 100.0ºC. (molar heat of vaporization of liquid water = 4.07 × 104 J/mol)

The forces that hold graphite, C(s), together in the solid state are

Which substance has the highest melting point?

What is the boiling point in °C of acetone at 1.2 atm?

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

Explain how a pressure cooker works by filling in the blanks in the following statement: A pressure cooker allows the pressure inside the cooker to become than atmospheric pressure, which the boiling point of the water used to cook the food, thus cooking the food .

HCl boils at -85°C and F₂ boils at -188°C. Which type of intermolecular force is responsible for the higher boiling point of HCl?

Calculate the amount of heat energy required to convert 27.5 g of water at 62.5°C to steam at 124.0°C. (C_water = 4.184 J/g°C; C_ice = 2.03 J/gºC; 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)

Calculate the amount of heat energy required to evaporate 27.5 g of water at 100.0ºC. (molar heat of vaporization of liquid water = 4.07 × 10⁴ J/mol)