Question 1

Define dynamic equilibrium.

Accepted Answer

Dynamic equilibrium

Question 2

How many compounds,of the ones listed below,have hydrogen bonding? CH3(CH2)2NH2 CH3(CH2)2NH(CH2)4CH3 (CH3CH2)2N(CH2)4CH3

Accepted Answer

A)  2 
B)  3 
C)  1 
D)  0 
A)  2 
B)  3 
C)  1 
D)  0

Question 3

Which of the following compounds exhibits hydrogen bonding?

Accepted Answer

A)  CH3Br 
B)  HCl  
C)  CH3SCH3 
D)  CH3OH  
A)  CH3Br 
B)  HCl  
C)  CH3SCH3 
D)  CH3OH

Question 4

Place the following substances in order of increasing boiling point. He I2 O2

Accepted Answer

A)  He 2  2 
B)  I2 2  2 2  2 2 
E)  He 2  2 
A)  He 2  2 
B)  I2 2  2 2  2 2 
E)  He 2  2

Question 5

Place the following substances in order of decreasing boiling point. He Ar H2

Accepted Answer

A)  He > H2  > Ar 
B)  H2 > He > Ar 
C)  He > Ar > H2 
D)  Ar > He > H2 
E)  H2 > Ar > He 
A)  He > H2  > Ar 
B)  H2 > He > Ar 
C)  He > Ar > H2 
D)  Ar > He > H2 
E)  H2 > Ar > He

Question 6

Explain why ice floats in water.

Accepted Answer

A)  Ice is more dense than water. 
B)  Steam is less dense than water. 
C)  Ice is less dense than water. 
D)  Steam is more dense than water. 
E)  Ice is the same density as water. 
A)  Ice is more dense than water. 
B)  Steam is less dense than water. 
C)  Ice is less dense than water. 
D)  Steam is more dense than water. 
E)  Ice is the same density as water.

Question 7

Determine ΔHvap for a compound that has a measured vapor pressure of 24.3 torr at 273 K and 135 torr at 325 K.

Accepted Answer

A)  41 kJ/mol 
B)  79 kJ/mol 
C)  24 kJ/mol 
D)  13 kJ/mol 
E)  34 kJ/mol 
A)  41 kJ/mol 
B)  79 kJ/mol 
C)  24 kJ/mol 
D)  13 kJ/mol 
E)  34 kJ/mol

Question 8

Define fusion.

Accepted Answer

A)  the phase transition from solid to liquid 
B)  the phase transition from gas to solid 
C)  the phase transition from gas to liquid 
D)  the phase transition from liquid to gas 
E)  the phase transition from liquid to solid 
A)  the phase transition from solid to liquid 
B)  the phase transition from gas to solid 
C)  the phase transition from gas to liquid 
D)  the phase transition from liquid to gas 
E)  the phase transition from liquid to solid

Question 9

Describe sweating in humans.

Accepted Answer

A)  It is an endothermic reaction. 
B)  The sweat evaporates absorbing heat from the body. 
C)  The skin is cooled. 
D)  None of the above 
E)  All of the above 
A)  It is an endothermic reaction. 
B)  The sweat evaporates absorbing heat from the body. 
C)  The skin is cooled. 
D)  None of the above 
E)  All of the above

Question 10

Identify the compound that does NOT have dipole-dipole forces as its strongest force.

Accepted Answer

A)  CH2I2 
B)  CH3OCH3 
C)  CH3Cl 
D)  HCBr3 
E)  CO2 
A)  CH2I2 
B)  CH3OCH3 
C)  CH3Cl 
D)  HCBr3 
E)  CO2

Question 11

Choose the molecule or compound that exhibits dispersion forces as its strongest intermolecular force.

Accepted Answer

A)  Cl2 
B)  CO 
C)  HBr 
D)  NaCl 
E)  All of these have intermolecular forces stronger than dispersion. 
A)  Cl2 
B)  CO 
C)  HBr 
D)  NaCl 
E)  All of these have intermolecular forces stronger than dispersion.

Question 12

Identify the compound that does NOT have hydrogen bonding.

Accepted Answer

A)  (CH3)2N(CH2)3CH3 
B)  H2O 
C)  CH3(CH2)5 
D)  HF 
E)  CH3(CH2)2NH2 
A)  (CH3)2N(CH2)3CH3 
B)  H2O 
C)  CH3(CH2)5 
D)  HF 
E)  CH3(CH2)2NH2

Question 13

Define deposition.

Accepted Answer

A)  A liquid becomes a gas. 
B)  A gas becomes a liquid. 
C)  A gas becomes a solid. 
D)  A solid becomes a gas. 
E)  A solid becomes a liquid. 
A)  A liquid becomes a gas. 
B)  A gas becomes a liquid. 
C)  A gas becomes a solid. 
D)  A solid becomes a gas. 
E)  A solid becomes a liquid.

Question 14

The forces between polar molecules are known as

Accepted Answer

A)  hydrogen bonding. 
B)  ion-dipole forces. 
C)  dipole-dipole forces. 
D)  dispersion forces. 
E)  ionic forces. 
A)  hydrogen bonding. 
B)  ion-dipole forces. 
C)  dipole-dipole forces. 
D)  dispersion forces. 
E)  ionic forces.

Question 15

Ethyl chloride,C2H5Cl,is used as a local anesthetic.It works by cooling tissue as it vaporizes; its heat of vaporization is 26.4 kJ/mol.How much heat could be removed by 10.0 g of ethyl chloride?

Accepted Answer

A)  4.09 kJ 
B)  170 kJ 
C)  264 kJ 
D)  1700 kJ 
A)  4.09 kJ 
B)  170 kJ 
C)  264 kJ 
D)  1700 kJ

Question 16

Which of the following statements is FALSE?

Accepted Answer

A)  The rate of vaporization increases with increasing surface area. 
B)  The rate of vaporization increases with decreasing strength of intermolecular forces. 
C)  The rate of vaporization increases with increasing temperature. 
D)  Molecules with hydrogen bonding are more volatile than compounds with dipole-dipole forces. 
E)  None of the above is false. 
A)  The rate of vaporization increases with increasing surface area. 
B)  The rate of vaporization increases with decreasing strength of intermolecular forces. 
C)  The rate of vaporization increases with increasing temperature. 
D)  Molecules with hydrogen bonding are more volatile than compounds with dipole-dipole forces. 
E)  None of the above is false.

Question 17

The melting point of water is ________.

Accepted Answer

A)  0°C 
B)  32 K 
C)  212°C 
D)  100°F 
E)  273°F 
A)  0°C 
B)  32 K 
C)  212°C 
D)  100°F 
E)  273°F

Question 18

Place the following substances in order of decreasing vapor pressure at a given temperature. BeF2 CH3OH OF2

Accepted Answer

A)  CH3OH > OF2  > BeF2 
B)  BeF2 > OF2  > CH3OH 
C)  OF2 > CH3OH > BeF2 
D)  OF2 > BeF2 > CH3OH 
E)  BeF2 > CH3OH > OF2 
A)  CH3OH > OF2  > BeF2 
B)  BeF2 > OF2  > CH3OH 
C)  OF2 > CH3OH > BeF2 
D)  OF2 > BeF2 > CH3OH 
E)  BeF2 > CH3OH > OF2

Question 19

How much energy is required to vaporize 98.6 g of ethanol (C2H5OH)at its boiling point,if its ΔHvap is 40.5 kJ/mol?

Accepted Answer

A)  86.7 kJ 
B)  11.5 kJ 
C)  18.9 kJ 
D)  52.8 kJ 
E)  39.9 kJ 
A)  86.7 kJ 
B)  11.5 kJ 
C)  18.9 kJ 
D)  52.8 kJ 
E)  39.9 kJ

Question 20

Identify the place which has the highest boiling point of water.

Accepted Answer

A)  Death Valley, 282 feet below sea level 
B)  A pressurized passenger jet, 39,000 feet 
C)  Panama City, Florida, sea level 
D)  Mt. Everest, 29,035 feet 
E)  Denver, Colorado, 5,280 feet 
A)  Death Valley, 282 feet below sea level 
B)  A pressurized passenger jet, 39,000 feet 
C)  Panama City, Florida, sea level 
D)  Mt. Everest, 29,035 feet 
E)  Denver, Colorado, 5,280 feet

Exam 11: Liquids,solids,and Intermolecular Forces

Define dynamic equilibrium.

How many compounds,of the ones listed below,have hydrogen bonding? CH3(CH2)2NH2 CH3(CH2)2NH(CH2)4CH3 (CH3CH2)2N(CH2)4CH3

Which of the following compounds exhibits hydrogen bonding?

Place the following substances in order of increasing boiling point. He I2 O2

Place the following substances in order of decreasing boiling point. He Ar H2

Explain why ice floats in water.

Determine ΔHvap for a compound that has a measured vapor pressure of 24.3 torr at 273 K and 135 torr at 325 K.

Define fusion.

Describe sweating in humans.

Identify the compound that does NOT have dipole-dipole forces as its strongest force.

Choose the molecule or compound that exhibits dispersion forces as its strongest intermolecular force.

Identify the compound that does NOT have hydrogen bonding.

Define deposition.

The forces between polar molecules are known as

Ethyl chloride,C2H5Cl,is used as a local anesthetic.It works by cooling tissue as it vaporizes; its heat of vaporization is 26.4 kJ/mol.How much heat could be removed by 10.0 g of ethyl chloride?

Which of the following statements is FALSE?

The melting point of water is ________.

Place the following substances in order of decreasing vapor pressure at a given temperature. BeF2 CH3OH OF2

How much energy is required to vaporize 98.6 g of ethanol (C2H5OH)at its boiling point,if its ΔHvap is 40.5 kJ/mol?

Identify the place which has the highest boiling point of water.

Matter, measurement, and Problem Solving

Atoms and Elements

Molecules,compounds,and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes,valence Bond Theory,

Solids and Modern Materials

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

How many compounds,of the ones listed below,have hydrogen bonding? CH₃(CH₂)₂NH₂ CH₃(CH₂)₂NH(CH₂)₄CH₃ (CH₃CH₂)₂N(CH₂)₄CH₃

Place the following substances in order of increasing boiling point. He I₂O₂

Place the following substances in order of decreasing boiling point. He Ar H₂

Determine ΔH_vap for a compound that has a measured vapor pressure of 24.3 torr at 273 K and 135 torr at 325 K.

Ethyl chloride,C₂H₅Cl,is used as a local anesthetic.It works by cooling tissue as it vaporizes; its heat of vaporization is 26.4 kJ/mol.How much heat could be removed by 10.0 g of ethyl chloride?

Place the following substances in order of decreasing vapor pressure at a given temperature. BeF₂ CH₃OH OF₂

How much energy is required to vaporize 98.6 g of ethanol (C₂H₅OH)at its boiling point,if its ΔH_vap is 40.5 kJ/mol?