Question 1

Which of the following compounds has the highest boiling point?

Accepted Answer

A) H2O 
B) H Cl 
C) H2S  
D) N H3 
A) H2O 
B) H Cl 
C) H2S  
D) N H3

Question 2

How much energy is required to heat 36.0 g H2O from a liquid at 65°C to a gas at 115°C? The following physical data may be useful.
ΔHvap = 40.7 kJ/mol
Cliq = 4.18 J/g°C
Cgas = 2.01 J/g°C
Csol = 2.09 J/g°C
Tmelting = 0°C
Tboiling = 100°C

Accepted Answer

A) 63.5 kJ 
B) 87.7 kJ 
C) 10.9 kJ 
D) 52.7 kJ 
E) 91.7 kJ 
A) 63.5 kJ 
B) 87.7 kJ 
C) 10.9 kJ 
D) 52.7 kJ 
E) 91.7 kJ

Question 3

Nickel has a face-centered cubic structure and has a density of 8.90 g/cm3.What is its atomic radius?

Accepted Answer

A) 125 pm 
B) 249 pm 
C) 353 pm 
D) 997 pm 
A) 125 pm 
B) 249 pm 
C) 353 pm 
D) 997 pm

Question 4

Match the following.
-LiI

Accepted Answer

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

Question 5

In the phase diagram,what is the triple point?

Accepted Answer

A) 114°C 
B) 184°C 
C) 535°C 
D) 128°C 
A) 114°C 
B) 184°C 
C) 535°C 
D) 128°C

Question 6

How many atoms are present in a body-centered cubic unit cell?

Accepted Answer

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

Question 7

The normal boiling point for H2Se is higher than the normal boiling point for H2S .This can be explained by

Accepted Answer

A) larger dipole-dipole forces for H2Se. 
B) larger dispersion forces for H2Se. 
C) larger hydrogen-bond forces for H2Se. 
D) larger dipole-dipole forces,larger dispersion forces,and larger hydrogen-bond forces for H2Se. 
A) larger dipole-dipole forces for H2Se. 
B) larger dispersion forces for H2Se. 
C) larger hydrogen-bond forces for H2Se. 
D) larger dipole-dipole forces,larger dispersion forces,and larger hydrogen-bond forces for H2Se.

Question 8

Assign the appropriate labels to the phase diagram shown below.

Accepted Answer

A) A = liquid,B = solid,C = gas,D = critical point 
B) A = gas,B = solid,C = liquid,D = triple point 
C) A = gas,B = liquid,C = solid,D = critical point 
D) A = solid,B = gas,C = liquid,D = supercritical fluid 
E) A = liquid,B = gas,C = solid,D = triple point 
A) A = liquid,B = solid,C = gas,D = critical point 
B) A = gas,B = solid,C = liquid,D = triple point 
C) A = gas,B = liquid,C = solid,D = critical point 
D) A = solid,B = gas,C = liquid,D = supercritical fluid 
E) A = liquid,B = gas,C = solid,D = triple point

Question 9

What is the strongest type of intermolecular force present in H2?

Accepted Answer

A) ion-dipole 
B) dipole-dipole 
C) dispersion 
D) hydrogen bonding 
E) None of the above 
A) ion-dipole 
B) dipole-dipole 
C) dispersion 
D) hydrogen bonding 
E) None of the above

Question 10

In liquid propanol,
CH3CH2CH2OH   
Which intermolecular forces are present?

Accepted Answer

A) Dispersion,hydrogen bonding and dipole-dipole forces are present. 
B) Only dipole-dipole and ion-dipole forces are present. 
C) Only dispersion and dipole-dipole forces are present. 
D) Only hydrogen bonding forces are present. 
A) Dispersion,hydrogen bonding and dipole-dipole forces are present. 
B) Only dipole-dipole and ion-dipole forces are present. 
C) Only dispersion and dipole-dipole forces are present. 
D) Only hydrogen bonding forces are present.

Question 11

Which of the following substances should have the highest melting point?

Accepted Answer

A) CO2 
B) SrS 
C) Xe 
D) F2 
E) MgO 
A) CO2 
B) SrS 
C) Xe 
D) F2 
E) MgO

Question 12

Which of the following is considered a molecular solid?

Accepted Answer

A) Cu 
B) NH4NO3 
C) I2 
D) Xe 
E) None of these is a molecular solid. 
A) Cu 
B) NH4NO3 
C) I2 
D) Xe 
E) None of these is a molecular solid.

Question 13

Choose the pair of substances that are most likely to form a homogeneous solution.

Accepted Answer

A) C6H14 and C10H20 
B) LiBr and C5H12 
C) N2O4 and NH4Cl 
D) C6H14 and H2O 
E) None of the pairs above will form a homogeneous solution. 
A) C6H14 and C10H20 
B) LiBr and C5H12 
C) N2O4 and NH4Cl 
D) C6H14 and H2O 
E) None of the pairs above will form a homogeneous solution.

Question 14

Choose the substance with the highest vapor pressure at a given temperature.

Accepted Answer

A) SiS2 
B) RbCl 
C) CH3SCH3 
D) BF3 
E) SbH3 
A) SiS2 
B) RbCl 
C) CH3SCH3 
D) BF3 
E) SbH3

Question 15

Give the phase transition that occurs as the temperature of dry ice increases.

Accepted Answer

A) from solid to gas 
B) from gas to solid 
C) from liquid to gas 
D) from liquid to solid 
E) from solid to liquid 
A) from solid to gas 
B) from gas to solid 
C) from liquid to gas 
D) from liquid to solid 
E) from solid to liquid

Question 16

Determine the vapor pressure (in mm Hg)of a substance at 29°C,whose normal boiling point is 76°C and has a ΔHvap of 38.7 kJ/mol.

Accepted Answer

A) 80 mm Hg 
B) 13 mm Hg 
C) 21 mm Hg 
D) 48 mm Hg 
E) 96 mm Hg 
A) 80 mm Hg 
B) 13 mm Hg 
C) 21 mm Hg 
D) 48 mm Hg 
E) 96 mm Hg

Question 17

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  
 And   Respectively.For H2O,∆Hfus = 6.01 kJ/mol,and ∆Hvap = 40.67 kJ/mol.

Accepted Answer

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

Question 18

Consider the phase diagram shown.Choose the statement below that is true.

Accepted Answer

A) The triple point of this substance occurs at a temperature of 31°C. 
B) At 10 atm of pressure,there is no temperature where the liquid phase of this substance would exist. 
C) The solid phase of this substance is higher in density than the liquid phase. 
D) The line separating the solid and liquid phases represents the ΔHvap. 
E) None of the above are true. 
A) The triple point of this substance occurs at a temperature of 31°C. 
B) At 10 atm of pressure,there is no temperature where the liquid phase of this substance would exist. 
C) The solid phase of this substance is higher in density than the liquid phase. 
D) The line separating the solid and liquid phases represents the ΔHvap. 
E) None of the above are true.

Question 19

Choose the substance with the lowest viscosity.

Accepted Answer

A) Cl3CCCl3 
B) Cl2CHCH2Cl 
C) Cl2CHCHCl2 
D) ClCH2CH2Cl 
E) Cl3CCHCl2 
A) Cl3CCCl3 
B) Cl2CHCH2Cl 
C) Cl2CHCHCl2 
D) ClCH2CH2Cl 
E) Cl3CCHCl2

Question 20

Which of the following compounds exhibits hydrogen bonding?

Accepted Answer

A) CH3I 
B) H2 
C) C6H5CH3 
D) CH3OH 
A) CH3I 
B) H2 
C) C6H5CH3 
D) CH3OH

Which of the following compounds has the highest boiling point?

How much energy is required to heat 36.0 g H₂O from a liquid at 65°C to a gas at 115°C? The following physical data may be useful. ΔH_vap = 40.7 kJ/mol C_liq = 4.18 J/g°C C_gas= 2.01 J/g°C C_sol = 2.09 J/g°C T_melting= 0°C T_boiling = 100°C

Nickel has a face-centered cubic structure and has a density of 8.90 g/cm³.What is its atomic radius?

Match the following. -LiI

In the phase diagram,what is the triple point?

How many atoms are present in a body-centered cubic unit cell?

The normal boiling point for H₂Seis higher than the normal boiling point for H₂S.This can be explained by

Assign the appropriate labels to the phase diagram shown below.

What is the strongest type of intermolecular force present in H₂?

In liquid propanol, CH₃CH₂CH₂OH Which intermolecular forces are present?

Which of the following substances should have the highest melting point?

Which of the following is considered a molecular solid?

Choose the pair of substances that are most likely to form a homogeneous solution.

Choose the substance with the highest vapor pressure at a given temperature.

Give the phase transition that occurs as the temperature of dry ice increases.

Determine the vapor pressure (in mm Hg)of a substance at 29°C,whose normal boiling point is 76°C and has a ΔH_vapof 38.7 kJ/mol.

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 And Respectively.For H₂O,∆H_fus= 6.01 kJ/mol,and ∆H_vap= 40.67 kJ/mol.

Consider the phase diagram shown.Choose the statement below that is true.

Choose the substance with the lowest viscosity.

Which of the following compounds exhibits hydrogen bonding?

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, and

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Filters

Exam 11: Liquids, Solids, and Intermolecular Forces

Which of the following compounds has the highest boiling point?

How much energy is required to heat 36.0 g H2O from a liquid at 65°C to a gas at 115°C? The following physical data may be useful. ΔHvap = 40.7 kJ/mol Cliq = 4.18 J/g°C Cgas = 2.01 J/g°C Csol = 2.09 J/g°C Tmelting = 0°C Tboiling = 100°C

Nickel has a face-centered cubic structure and has a density of 8.90 g/cm3.What is its atomic radius?

Match the following. -LiI

In the phase diagram,what is the triple point?

How many atoms are present in a body-centered cubic unit cell?

The normal boiling point for H2Se is higher than the normal boiling point for H2S .This can be explained by

Assign the appropriate labels to the phase diagram shown below.

What is the strongest type of intermolecular force present in H2?

In liquid propanol, CH3CH2CH2OH Which intermolecular forces are present?

Which of the following substances should have the highest melting point?

Which of the following is considered a molecular solid?

Choose the pair of substances that are most likely to form a homogeneous solution.

Choose the substance with the highest vapor pressure at a given temperature.

Give the phase transition that occurs as the temperature of dry ice increases.

Determine the vapor pressure (in mm Hg)of a substance at 29°C,whose normal boiling point is 76°C and has a ΔHvap of 38.7 kJ/mol.

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 And Respectively.For H2O,∆Hfus = 6.01 kJ/mol,and ∆Hvap = 40.67 kJ/mol.

Consider the phase diagram shown.Choose the statement below that is true.

Choose the substance with the lowest viscosity.

Which of the following compounds exhibits hydrogen bonding?

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, and

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Filters

How much energy is required to heat 36.0 g H₂O from a liquid at 65°C to a gas at 115°C? The following physical data may be useful. ΔH_vap = 40.7 kJ/mol C_liq = 4.18 J/g°C C_gas= 2.01 J/g°C C_sol = 2.09 J/g°C T_melting= 0°C T_boiling = 100°C

Nickel has a face-centered cubic structure and has a density of 8.90 g/cm³.What is its atomic radius?

The normal boiling point for H₂Seis higher than the normal boiling point for H₂S.This can be explained by

What is the strongest type of intermolecular force present in H₂?

In liquid propanol, CH₃CH₂CH₂OH Which intermolecular forces are present?

Determine the vapor pressure (in mm Hg)of a substance at 29°C,whose normal boiling point is 76°C and has a ΔH_vapof 38.7 kJ/mol.

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 And Respectively.For H₂O,∆H_fus= 6.01 kJ/mol,and ∆H_vap= 40.67 kJ/mol.