Question 1

Of the following, is an exothermic process.
Melting subliming freezing boiling

Accepted Answer

A)  freezing 
B)  boiling 
C)  subliming 
D)  melting 
E)  All of the above are exothermic. 
A)  freezing 
B)  boiling 
C)  subliming 
D)  melting 
E)  All of the above are exothermic.

Question 2

Of the following substances, only has London dispersion forces as its only intermolecular force.

Accepted Answer

A)  CH3OH 
B)  CH4  
C)  NH3  
D)  HCl 
E)  H2S 
A)  CH3OH 
B)  CH4  
C)  NH3  
D)  HCl 
E)  H2S

Question 3

The fluorocarbon C2Cl3F3 has a normal boiling point of 47.6°C. The specific heats of C2Cl3F3 (l) and C2Cl3F3(g) are 0.91 J/g- K and 0.67 J/g- K, respectively. The heat of vaporization of the compound is 27.49 kJ/mol. The heat required to convert 50.0 g of the compound from the liquid at 5.0°C to the gas at 80.0°C is kJ.

Accepted Answer

A)  1454 
B)  10.36 
C)  30.51 
D)  3031 
E)  8.19 
A)  1454 
B)  10.36 
C)  30.51 
D)  3031 
E)  8.19

Question 4

On a phase diagram, the critical pressure is .

Accepted Answer

A)  the pressure above which a substance is a liquid at all temperatures 
B)  the pressure at which a liquid changes to a gas 
C)  the pressure required to melt a solid 
D)  the pressure required to liquefy a gas at its critical temperature 
E)  the pressure below which a substance is a solid at all temperatures 
A)  the pressure above which a substance is a liquid at all temperatures 
B)  the pressure at which a liquid changes to a gas 
C)  the pressure required to melt a solid 
D)  the pressure required to liquefy a gas at its critical temperature 
E)  the pressure below which a substance is a solid at all temperatures

Question 5

NaCl crystallizes in a face- centered cubic cell. What is the total number of ions (Na+ ions and Cl- ions) that lie within a unit cell of NaCl?

Accepted Answer

A)  6 
B)  2 
C)  4 
D)  8 
E)  5 
A)  6 
B)  2 
C)  4 
D)  8 
E)  5

Question 6

What intermolecular force is responsible for the fact that ice is less dense than liquid water?

Accepted Answer

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

Question 7

The heat of fusion of water is 6.01 kJ/mol. The heat capacity of liquid water is 75.3 J/mol · K. The conversion of 50.0 g of ice at 0.00°C to liquid water at 22.0°C requires kJ of heat.

Accepted Answer

A)  17.2 
B)  3.8 × 102 
C)  0.469 
D)  21.3 
E)  Insufficient data are given. 
A)  17.2 
B)  3.8 × 102 
C)  0.469 
D)  21.3 
E)  Insufficient data are given.

Question 8

The enthalpy change for converting 10.0 g of ice at - 25.0°C to water at 80.0°C is kJ. The specific heats of ice, water, and steam are 2.09 J/g- K, 4.18 J/g- K, and 1.84 J/g- K, respectively. For H2O, OHfus = 6.01 kJ/mol, and OHvap = 40.67 kJ/mol

Accepted Answer

A)  6.16 
B)  9.88 
C)  3870 
D)  7.21 
E)  12.28 
A)  6.16 
B)  9.88 
C)  3870 
D)  7.21 
E)  12.28

Question 9

Of the following substances, _ has the highest boiling point.

Accepted Answer

A)  H2O 
B)  Kr 
C)  CH4  
D)  CO2  
E)  NH3 
A)  H2O 
B)  Kr 
C)  CH4  
D)  CO2  
E)  NH3

Question 10

Some things take longer to cook at high altitudes than at low altitudes because .

Accepted Answer

A)  water boils at a higher temperature at high altitude than at low altitude 
B)  water boils at a lower temperature at high altitude than at low altitude 
C)  there is a higher moisture content in the air at high altitude 
D)  heat isn't conducted as well in low density air 
E)  natural gas flames don't burn as hot at high altitudes 
A)  water boils at a higher temperature at high altitude than at low altitude 
B)  water boils at a lower temperature at high altitude than at low altitude 
C)  there is a higher moisture content in the air at high altitude 
D)  heat isn't conducted as well in low density air 
E)  natural gas flames don't burn as hot at high altitudes

Question 11

What is the predominant intermolecular force in CBr4?

Accepted Answer

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

Question 12

A solid has a very high melting point, great hardness, and poor electrical conduction. This is a(n)
Solid.

Accepted Answer

A)  metallic and covalent network 
B)  covalent network 
C)  molecular 
D)  metallic 
E)  ionic 
A)  metallic and covalent network 
B)  covalent network 
C)  molecular 
D)  metallic 
E)  ionic

Question 13

How many atoms are contained in a face- centered cubic unit cell?

Accepted Answer

The answer of How many atoms are contained in a...

Question 14

The enthalpy change for converting 1.00 mol of ice at - 50.0°C to water at 70.0°C is kJ. The specific heats of ice, water, and steam are 2.09 J/g- K, 4.18 J/g- K, and 1.84 J/g- K, respectively. For H2O, OHfus = 6.01 kJ/mol, and OHvap = 40.67 kJ/mol

Accepted Answer

A)  12.28 
B)  13.16 
C)  6.41 
D)  9.40 
E)  7154 
A)  12.28 
B)  13.16 
C)  6.41 
D)  9.40 
E)  7154

Question 15

On the phase diagram shown, the coordinates of point correspond to the critical temperature and pressure.

Accepted Answer

A)  A 
B)  B 
C)  C 
D)  D 
E)  E 
A)  A 
B)  B 
C)  C 
D)  D 
E)  E

Question 16

Which one of the following derivatives of ethane has the highest boiling point?

Accepted Answer

A)  C2F6  
B)  C2Cl6  
C)  C2Br6  
D)  C2H6  
E)  C2I6 
A)  C2F6  
B)  C2Cl6  
C)  C2Br6  
D)  C2H6  
E)  C2I6

Question 17

The heating curve shown was generated by measuring the heat flow and temperature for a solid as it was heated. The slope of the segment corresponds to the heat capacity of the solid.

Accepted Answer

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

Question 18

On a phase diagram, the critical temperature is .

Accepted Answer

A)  the temperature below which a gas cannot be liquefied 
B)  the temperature required to melt a solid 
C)  the temperature above which a gas cannot be liquefied 
D)  the temperature at which all three states are in equilibrium 
E)  the temperature required to cause sublimation of a solid 
A)  the temperature below which a gas cannot be liquefied 
B)  the temperature required to melt a solid 
C)  the temperature above which a gas cannot be liquefied 
D)  the temperature at which all three states are in equilibrium 
E)  the temperature required to cause sublimation of a solid

Question 19

The phase diagram of a substance is shown above. The area labeled indicates the gas phase for the substance.

Accepted Answer

A)  w 
B)  x 
C)  y 
D)  z 
E)  y and z 
A)  w 
B)  x 
C)  y 
D)  z 
E)  y and z

Question 20

Ethanol (C2H5OH) melts at - 114°C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g- K and 2.3 J/g- K, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at - 135°C to liquid ethanol at - 50°C?

Accepted Answer

A)  207.3 
B)  9.21 
C)  - 12.7 
D)  6.91 
E)  4192 
A)  207.3 
B)  9.21 
C)  - 12.7 
D)  6.91 
E)  4192

Exam 11: Intermolecular Forces, Liquids, and Solids

Of the following, is an exothermic process. Melting subliming freezing boiling

Of the following substances, only has London dispersion forces as its only intermolecular force.

On a phase diagram, the critical pressure is .

NaCl crystallizes in a face- centered cubic cell. What is the total number of ions (Na+ ions and Cl- ions) that lie within a unit cell of NaCl?

What intermolecular force is responsible for the fact that ice is less dense than liquid water?

The heat of fusion of water is 6.01 kJ/mol. The heat capacity of liquid water is 75.3 J/mol · K. The conversion of 50.0 g of ice at 0.00°C to liquid water at 22.0°C requires kJ of heat.

The enthalpy change for converting 10.0 g of ice at - 25.0°C to water at 80.0°C is kJ. The specific heats of ice, water, and steam are 2.09 J/g- K, 4.18 J/g- K, and 1.84 J/g- K, respectively. For H2O, OHfus = 6.01 kJ/mol, and OHvap = 40.67 kJ/mol

Of the following substances, _ has the highest boiling point.

Some things take longer to cook at high altitudes than at low altitudes because .

What is the predominant intermolecular force in CBr4?

A solid has a very high melting point, great hardness, and poor electrical conduction. This is a(n) Solid.

How many atoms are contained in a face- centered cubic unit cell?

The enthalpy change for converting 1.00 mol of ice at - 50.0°C to water at 70.0°C is kJ. The specific heats of ice, water, and steam are 2.09 J/g- K, 4.18 J/g- K, and 1.84 J/g- K, respectively. For H2O, OHfus = 6.01 kJ/mol, and OHvap = 40.67 kJ/mol

On the phase diagram shown, the coordinates of point correspond to the critical temperature and pressure.

Which one of the following derivatives of ethane has the highest boiling point?

The heating curve shown was generated by measuring the heat flow and temperature for a solid as it was heated. The slope of the segment corresponds to the heat capacity of the solid.

On a phase diagram, the critical temperature is .

The phase diagram of a substance is shown above. The area labeled indicates the gas phase for the substance.

Ethanol (C2H5OH) melts at - 114°C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g- K and 2.3 J/g- K, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at - 135°C to liquid ethanol at - 50°C?

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Gases

Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Chemistry of Coordination Compounds

The Chemistry of Life: Organic and Biological Chemistry

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NaCl crystallizes in a face- centered cubic cell. What is the total number of ions (Na⁺ions and Cl^- ions) that lie within a unit cell of NaCl?

The enthalpy change for converting 10.0 g of ice at - 25.0°C to water at 80.0°C is kJ. The specific heats of ice, water, and steam are 2.09 J/g- K, 4.18 J/g- K, and 1.84 J/g- K, respectively. For H₂O, OH_fus= 6.01 kJ/mol, and OH_vap= 40.67 kJ/mol

What is the predominant intermolecular force in CBr₄?

The enthalpy change for converting 1.00 mol of ice at - 50.0°C to water at 70.0°C is kJ. The specific heats of ice, water, and steam are 2.09 J/g- K, 4.18 J/g- K, and 1.84 J/g- K, respectively. For H₂O, OH_fus= 6.01 kJ/mol, and OH_vap= 40.67 kJ/mol

Ethanol (C₂H₅OH) melts at - 114°C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g- K and 2.3 J/g- K, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at - 135°C to liquid ethanol at - 50°C?