Question 1

Identify the substance with the highest viscosity in the liquid phase.

Accepted Answer

A) gasoline 
B) water 
C) corn syrup 
D) motor oil 
E) tea

Question 2

Consider the phase diagram below. If the dashed line at 1 atm of pressure is followed from 100 to 500 °C, what phase changes will occur (in order of increasing temperature)?

Accepted Answer

A) condensation followed by vaporization 
B) sublimation followed by deposition 
C) vaporization followed by deposition 
D) fusion followed by vaporization 
E) No phase change will occur under the conditions specified.

Question 3

What is the strongest type of intermolecular force present in CHF3?

Accepted Answer

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

Question 4

Give the term for the temperature at which the gas and liquid phases form a supercritical fluid.

Accepted Answer

A) absolute temperature 
B) definite temperature 
C) fluid temperature 
D) critical temperature 
E) solid temperature

Question 5

Which is expected to have the largest dispersion forces?

Accepted Answer

A) C3H8 
B) C12H26 
C) F2 
D) Be Cl2

Question 6

The freezing point of water is ________.

Accepted Answer

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

Question 7

Why is the Δ_vapH higher than Δ_fusHfor a given compound?

Accepted Answer

The answer of Why is the Δ_vapH higher than Δ_fusH_...

Question 8

Define dynamic equilibrium between the liquid and gaseous phases.

Accepted Answer

The answer of Define dynamic equilibrium between the liquid and...

Question 9

Place the following substances in order of increasing vapour pressure at a given temperature. NF3 NH3 BCl3

Accepted Answer

A) NH3 3 3 
B) NF3 3 3 
C) BCl3 3 3 
D) NH3 3 3 
E) BCl3 3 3

Question 10

The heat of vaporization of water at 100 °C is 40.66 kJ mol-1. Calculate the quantity of heat that is absorbed/released when 9.00 g of steam condenses to liquid water at 100 °C.

Accepted Answer

A) 20.3 kJ of heat are absorbed. 
B) 20.3 kJ of heat are released. 
C) 81.3 kJ of heat are absorbed. 
D) 81.3 kJ of heat are released.

Question 11

In liquid ethanol, CH3CH2OH 
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.

Question 12

Match the following.

-CH3CH3

Accepted Answer

A) dispersion forces 
B) dipole-dipole forces 
C) ion-dipole forces 
D) hydrogen bonding 
E) ionic bond
F)H2 + H2O

Question 13

Identify triple point.

Accepted Answer

A) the temperature, pressure, and density for a gas 
B) the temperature at which the boiling point equals the melting point 
C) the temperature and pressure where liquid, solid, and gas are equally stable and are in equilibrium 
D) the temperature that is unique for a substance 
E) the temperature at which the solid and liquid coexist

Question 14

Identify the type of solid for argon.

Accepted Answer

A) metallic atomic solid 
B) ionic solid 
C) nonbonding atomic solid 
D) molecular solid 
E) networking atomic solid

Question 15

Define sublimation.

Accepted Answer

A) the phase transition from solid to gas 
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 16

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

Accepted Answer

A) H2 
B) SO2 
C) NH3 
D) CF4 
E) BCl3

Question 17

Choose the substance with the highest surface tension in the liquid phase.

Accepted Answer

A) HOCH2CH2OH 
B) CH2F2 
C) CH3CH2F 
D) CH3CH2OH 
E) CH3CH2CH3

Question 18

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-1 °C-1, 4.18 J g-1 °C-1, and 1.84 J g-1 °C-1, respectively. For H2O, ΔfusH = 6.01 kJ mol-1, and ΔvapH = 40.67 kJ mol-1.

Accepted Answer

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

Question 19

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

Accepted Answer

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

Question 20

Which of the following compounds has the highest boiling point?

Accepted Answer

A) H2O 
B) HI 
C) H2Te  
D) AsH3

Exam 11: Liquids, Solids, and Intermolecular Forces

Identify the substance with the highest viscosity in the liquid phase.

Consider the phase diagram below. If the dashed line at 1 atm of pressure is followed from 100 to 500 °C, what phase changes will occur (in order of increasing temperature) ?

What is the strongest type of intermolecular force present in CHF₃?

Give the term for the temperature at which the gas and liquid phases form a supercritical fluid.

Which is expected to have the largest dispersion forces?

The freezing point of water is ________.

Why is the Δ_vapH higher than Δ_fusHfor a given compound?

Define dynamic equilibrium between the liquid and gaseous phases.

Place the following substances in order of increasing vapour pressure at a given temperature. NF₃ NH₃BCl₃

The heat of vaporization of water at 100 °C is 40.66 kJ mol^-1. Calculate the quantity of heat that is absorbed/released when 9.00 g of steam condenses to liquid water at 100 °C.

In liquid ethanol, CH₃CH₂OH Which intermolecular forces are present?

Match the following. -CH₃CH₃

Identify triple point.

Identify the type of solid for argon.

Define sublimation.

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

Choose the substance with the highest surface tension in the liquid phase.

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^-1 °C^-1, 4.18 J g^-1 °C^-1, and 1.84 J g^-1 °C^-1, respectively. For H₂O, Δ_fusH = 6.01 kJ mol^-1, and Δ_vapH = 40.67 kJ mol^-1.

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

Which of the following compounds has the highest boiling point?

Exam 11: Liquids, Solids, and Intermolecular Forces

Identify the substance with the highest viscosity in the liquid phase.

Consider the phase diagram below. If the dashed line at 1 atm of pressure is followed from 100 to 500 °C, what phase changes will occur (in order of increasing temperature) ?

What is the strongest type of intermolecular force present in CHF3?

Give the term for the temperature at which the gas and liquid phases form a supercritical fluid.

Which is expected to have the largest dispersion forces?

The freezing point of water is ________.

Why is the ΔvapH higher than ΔfusH for a given compound?

Define dynamic equilibrium between the liquid and gaseous phases.

Place the following substances in order of increasing vapour pressure at a given temperature. NF3 NH3 BCl3

The heat of vaporization of water at 100 °C is 40.66 kJ mol-1. Calculate the quantity of heat that is absorbed/released when 9.00 g of steam condenses to liquid water at 100 °C.

In liquid ethanol, CH3CH2OH Which intermolecular forces are present?

Match the following. -CH3CH3

Identify triple point.

Identify the type of solid for argon.

Define sublimation.

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

Choose the substance with the highest surface tension in the liquid phase.

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-1 °C-1, 4.18 J g-1 °C-1, and 1.84 J g-1 °C-1, respectively. For H2O, ΔfusH = 6.01 kJ mol-1, and ΔvapH = 40.67 kJ mol-1.

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

Which of the following compounds has the highest boiling point?

What is the strongest type of intermolecular force present in CHF₃?

Why is the Δ_vapH higher than Δ_fusHfor a given compound?

Place the following substances in order of increasing vapour pressure at a given temperature. NF₃ NH₃BCl₃

The heat of vaporization of water at 100 °C is 40.66 kJ mol^-1. Calculate the quantity of heat that is absorbed/released when 9.00 g of steam condenses to liquid water at 100 °C.

In liquid ethanol, CH₃CH₂OH Which intermolecular forces are present?

Match the following. -CH₃CH₃

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^-1 °C^-1, 4.18 J g^-1 °C^-1, and 1.84 J g^-1 °C^-1, respectively. For H₂O, Δ_fusH = 6.01 kJ mol^-1, and Δ_vapH = 40.67 kJ mol^-1.