Question 1

Which one of the following substances should exhibit hydrogen bonding in the liquid state

Accepted Answer

A)  PH3 
B)  He 
C)  H2S 
D)  CH4 
E)  CH3OH 
A)  PH3 
B)  He 
C)  H2S 
D)  CH4 
E)  CH3OH

Question 2

Indicate all the types of intermolecular forces of attraction in C2H6(g).

Accepted Answer

A)  Dispersion and Dipole-dipole 
B)  Dipole-dipole and Ionic 
C)  Ion-dipole and Hydrogen bonding 
D)  Hydrogen bonding and Dispersion 
E)  Dispersion 
A)  Dispersion and Dipole-dipole 
B)  Dipole-dipole and Ionic 
C)  Ion-dipole and Hydrogen bonding 
D)  Hydrogen bonding and Dispersion 
E)  Dispersion

Question 3

The specific heat of liquid ethanol, C2H5OH(l), is 2.46 J/g·$\circ$C and the heat of vaporization is 39.3 kJ/mol. The boiling point of ethanol is 78.3 $\circ$C. What amount of enthalpy is required to heat 50.0 g of liquid ethanol from 23.0 $\circ$C to ethanol vapor at 78.3 $\circ$C

Accepted Answer

A)  42.7 kJ 
B)  49.5 kJ 
C)  179 kJ 
D)  1970kJ 
E)  6840 kJ 
A)  42.7 kJ 
B)  49.5 kJ 
C)  179 kJ 
D)  1970kJ 
E)  6840 kJ

Question 4

Potassium crystallizes in a body-centered cubic lattice. How many atoms are there per unit cell

Accepted Answer

A)  1 
B)  2 
C)  4 
D)  6 
E)  8 
A)  1 
B)  2 
C)  4 
D)  6 
E)  8

Question 5

Methane has a heat of fusion of 0.84 kJ/mol and a heat of vaporization of 9.2 kJ/mol. Estimate the value for the heat of sublimation.

Accepted Answer

A)  12.0 kJ/mol 
B)  11.0 kJ/mol 
C)  10.0 kJ/mol 
D)  9.00 kJ/mol 
E)  8.00 kJ/mol 
A)  12.0 kJ/mol 
B)  11.0 kJ/mol 
C)  10.0 kJ/mol 
D)  9.00 kJ/mol 
E)  8.00 kJ/mol

Question 6

How much energy (heat) is required to convert 52.0 g of ice at -10.0$\circ$C to steam at 100$\circ$C

specific heat of ice: $ \quad 2.09 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C} \quad \Delta \mathrm{H}_{\mathrm{fus}}=6.02 \mathrm{~kJ} / \mathrm{mol} $ 
specific heat of water: $ 4.18 \mathrm{~J} / \mathrm{g}{ \cdot}^{\circ} \mathrm{C} \quad \Delta \mathrm{H}_{\mathrm{vap}}=40.7 \mathrm{~kJ} / \mathrm{mo} $. 
specific heat of steam: $ 1.84 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C} $

Accepted Answer

A)  40.2 kJ 
B)  157.8 kJ 
C)  1,086 kJ 
D)  2,570 kJ 
E)  22,957 kJ 
A)  40.2 kJ 
B)  157.8 kJ 
C)  1,086 kJ 
D)  2,570 kJ 
E)  22,957 kJ

Question 7

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

Accepted Answer

A)  a low heat of vaporization 
B)  a low critical temperature 
C)  a low vapor pressure 
D)  a low boiling point 
E)  None of the above. 
A)  a low heat of vaporization 
B)  a low critical temperature 
C)  a low vapor pressure 
D)  a low boiling point 
E)  None of the above.

Question 8

Osmium tetroxide, OsO4, is a soft crystal that melts at 40$\circ$C. The liquid does not conduct electricity. What kind of crystal is this

Accepted Answer

A)  Ionic Crystal 
B)  Covalent Crystal 
C)  Metallic Crystal 
D)  Molecular Crystal 
E)  Amorphous (Not a regular crystal) 
A)  Ionic Crystal 
B)  Covalent Crystal 
C)  Metallic Crystal 
D)  Molecular Crystal 
E)  Amorphous (Not a regular crystal)

Question 9

Arrange the following substances in order of increasing boiling point: CH3OH, He, CH3Cl, and N2

Accepted Answer

A)  CH3OH 3Cl 2 
B)  He 2 3OH 3Cl 
C)  N2 3OH 3Cl 
D)  He 2 3Cl 3OH 
E)  CH3Cl 2 3OH 
A)  CH3OH 3Cl 2 
B)  He 2 3OH 3Cl 
C)  N2 3OH 3Cl 
D)  He 2 3Cl 3OH 
E)  CH3Cl 2 3OH

Question 10

The intermolecular forces present in CO include which of the following
I. dipole-dipole
II. ion-dipole
III. dispersion
IV. hydrogen bonding

Accepted Answer

A)  I, II, III, and IV 
B)  I and III 
C)  I, III, and IV 
D)  I and II 
E)  II and IV 
A)  I, II, III, and IV 
B)  I and III 
C)  I, III, and IV 
D)  I and II 
E)  II and IV

Question 11

Based on the phase diagram shown below, the solid phase is more dense than the liquid phase.

Accepted Answer

A) True 
 B)False

Question 12

The normal boiling point of methanol (CH3OH) is 64.6$\circ$C. Given that the vapor pressure of methanol is 75.0 torr at 15.2$\circ$C, calculate the molar enthalpy of vaporization of methanol.

Accepted Answer

A)  0.383 kJ/mol 
B)  3.00 kJ/mol 
C)  27.5 kJ/mol 
D)  38.0 kJ/mol 
E)  74.7 kJ/mol 
A)  0.383 kJ/mol 
B)  3.00 kJ/mol 
C)  27.5 kJ/mol 
D)  38.0 kJ/mol 
E)  74.7 kJ/mol

Question 13

The density of ice is less than the density of liquid water due to the formation of hydrogen bonds.

Accepted Answer

A) True 
 B)False

Question 14

Which one of the following substances crystallizes as a covalent crystal

Accepted Answer

A)  CaO 
B)  SiO2 
C)  CO2 
D)  Pb 
E)  KMnO4 
A)  CaO 
B)  SiO2 
C)  CO2 
D)  Pb 
E)  KMnO4

Question 15

Which of the following substances is expected to have the highest molar heat of vaporization ($\Delta$Hvap)

Accepted Answer

A)  Ar 
B)  C6H6 
C)  He 
D)  NH3 
E)  H2O 
A)  Ar 
B)  C6H6 
C)  He 
D)  NH3 
E)  H2O

Question 16

SrF2 crystallizes such that the Sr2+ ions are in a face-centered cubic arrangement and the F- ions are in the holes of the lattice (fluorite structure). How many F- ions are present in one unit cell of this crystal

Accepted Answer

A)  1 
B)  2 
C)  4 
D)  6 
E)  8 
A)  1 
B)  2 
C)  4 
D)  6 
E)  8

Question 17

What mass of water would need to evaporate from your skin in order to dissipate 1.7 * 105 J of heat from your body
H2O(l) $\rarr$ H2O(g) $\Delta$Hvap = 40.7 kJ/mol

Accepted Answer

A)  58.4 g 
B)  75.2 g 
C)  418 g 
D)  7.52 * 104 g 
E)  6.92 * 106 g 
A)  58.4 g 
B)  75.2 g 
C)  418 g 
D)  7.52 * 104 g 
E)  6.92 * 106 g

Question 18

A liquid boils when its

Accepted Answer

A)  vapor pressure is exactly 1 atmosphere. 
B)  vapor pressure is equal to, or greater than, the external pressure pushing on it. 
C)  temperature is equal to 273 K (standard temperature). 
D)  temperature is greater than room temperature. 
A)  vapor pressure is exactly 1 atmosphere. 
B)  vapor pressure is equal to, or greater than, the external pressure pushing on it. 
C)  temperature is equal to 273 K (standard temperature). 
D)  temperature is greater than room temperature.

Question 19

Which one of the following substances crystallizes as a molecular solid

Accepted Answer

A)  KI 
B)  SiO2 
C)  Sn 
D)  CH3OH 
E)  Al2(SO4)3 
A)  KI 
B)  SiO2 
C)  Sn 
D)  CH3OH 
E)  Al2(SO4)3

Question 20

A phase change from the gas phase directly to the solid phase is called:

Accepted Answer

A)  Sublimation 
B)  Condensation 
C)  Freezing 
D)  Melting 
E)  Deposition 
A)  Sublimation 
B)  Condensation 
C)  Freezing 
D)  Melting 
E)  Deposition

Exam 11: Intermolecular Forces and Liquids and Solids

Which one of the following substances should exhibit hydrogen bonding in the liquid state

Indicate all the types of intermolecular forces of attraction in C2H6(g).

Potassium crystallizes in a body-centered cubic lattice. How many atoms are there per unit cell

Methane has a heat of fusion of 0.84 kJ/mol and a heat of vaporization of 9.2 kJ/mol. Estimate the value for the heat of sublimation.

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

Osmium tetroxide, OsO4, is a soft crystal that melts at 40 ∘\circ∘ C. The liquid does not conduct electricity. What kind of crystal is this

Arrange the following substances in order of increasing boiling point: CH3OH, He, CH3Cl, and N2

The intermolecular forces present in CO include which of the following I. dipole-dipole II. ion-dipole III. dispersion IV. hydrogen bonding

Based on the phase diagram shown below, the solid phase is more dense than the liquid phase.

The normal boiling point of methanol (CH3OH) is 64.6 ∘\circ∘ C. Given that the vapor pressure of methanol is 75.0 torr at 15.2 ∘\circ∘ C, calculate the molar enthalpy of vaporization of methanol.

The density of ice is less than the density of liquid water due to the formation of hydrogen bonds.

Which one of the following substances crystallizes as a covalent crystal

Which of the following substances is expected to have the highest molar heat of vaporization ( Δ\DeltaΔ Hvap)

SrF2 crystallizes such that the Sr2+ ions are in a face-centered cubic arrangement and the F- ions are in the holes of the lattice (fluorite structure). How many F- ions are present in one unit cell of this crystal

What mass of water would need to evaporate from your skin in order to dissipate 1.7 * 105 J of heat from your body H2O(l) →\rarr→ H2O(g) Δ\DeltaΔ Hvap = 40.7 kJ/mol

A liquid boils when its

Which one of the following substances crystallizes as a molecular solid

A phase change from the gas phase directly to the solid phase is called:

Chemistry: The Study of Change

Atoms Molecules and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metals Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

Indicate all the types of intermolecular forces of attraction in C₂H₆(g).

Osmium tetroxide, OsO₄, is a soft crystal that melts at 40^$\circ$C. The liquid does not conduct electricity. What kind of crystal is this

Arrange the following substances in order of increasing boiling point: CH₃OH, He, CH₃Cl, and N₂

The normal boiling point of methanol (CH₃OH) is 64.6^$\circ$C. Given that the vapor pressure of methanol is 75.0 torr at 15.2^$\circ$C, calculate the molar enthalpy of vaporization of methanol.

Which of the following substances is expected to have the highest molar heat of vaporization ( $\Delta$ H_vap)

SrF₂ crystallizes such that the Sr²⁺ ions are in a face-centered cubic arrangement and the F^- ions are in the holes of the lattice (fluorite structure). How many F^- ions are present in one unit cell of this crystal

What mass of water would need to evaporate from your skin in order to dissipate 1.7 * 10⁵ J of heat from your body H₂O(l) $\rarr$ H₂O(g) $\Delta$ H_vap = 40.7 kJ/mol