Question 1

In the solid state disruptive forces are ________.

Accepted Answer

A)  roughly of the same magnitude as cohesive forces 
B)  very weak compared to cohesive forces 
C)  dominant over cohesive forces 
D)  a consequence of excessive potential energy. 
A)  roughly of the same magnitude as cohesive forces 
B)  very weak compared to cohesive forces 
C)  dominant over cohesive forces 
D)  a consequence of excessive potential energy.

Question 2

What is the heat of vaporization in J/g of an unknown liquid if 6823 J of heat are required to vaporize 58.0 g of the unknown at its boiling point?

Accepted Answer

A)  516 J/g 
B)  118 J/g 
C)  981 J/g 
D)  28,100 J/g 
A)  516 J/g 
B)  118 J/g 
C)  981 J/g 
D)  28,100 J/g

Question 3

Which of the following pairs of quantities is needed in calculating the amount of heat energy needed to change liquid water at 75 °C to steam at 110 °C?

Accepted Answer

A)  specific heat of water, specific heat of steam, and heat of vaporization for water 
B)  specific heat of ice and heat of fusion for water 
C)  heat of fusion for water and heat of condensation for water 
D)  specific heat of ice and specific heat of water 
A)  specific heat of water, specific heat of steam, and heat of vaporization for water 
B)  specific heat of ice and heat of fusion for water 
C)  heat of fusion for water and heat of condensation for water 
D)  specific heat of ice and specific heat of water

Question 4

How much heat energy is needed to convert 10.0 g of ice at ?10 °C to liquid water at 10 °C?
Specific heat of ice = 2.09 J/(g°C) Heat of fusion of ice = 334 J/g Specific heat of water = 4.18 J/g°C

Accepted Answer

A)  5270 J 
B)  1,070 J 
C)  6,210 J 
D)  3960 J 
A)  5270 J 
B)  1,070 J 
C)  6,210 J 
D)  3960 J

Question 5

Use a dashed line to illustrate hydrogen bonding between a methanol molecule and a hydrogen fluoride molecule.

Accepted Answer

The answer of Use a dashed line to illustrate hydrogen...

Question 6

Gases are highly compressible because the particles ________.

Accepted Answer

A)  strongly repel each other 
B)  have no potential energy 
C)  are very far apart 
D)  vibrate too much to be compressed 
A)  strongly repel each other 
B)  have no potential energy 
C)  are very far apart 
D)  vibrate too much to be compressed

Question 7

A nonvolatile liquid would ________.

Accepted Answer

A)  have weak attractive forces between molecules 
B)  have a high vapor pressure at room temperature 
C)  be a very "explosive" substance 
D)  have strong attractive forces between molecules 
A)  have weak attractive forces between molecules 
B)  have a high vapor pressure at room temperature 
C)  be a very "explosive" substance 
D)  have strong attractive forces between molecules

Question 8

How much energy is required to change 12.9 g of solid Cu to molten Cu at 1083 °C (melting point)?
Heat of fusion for Cu = 205 J/g

Accepted Answer

A)  1390 
B)  3150 
C)  2640 
D)  1990 
A)  1390 
B)  3150 
C)  2640 
D)  1990

Question 9

Which of the following would have the same numerical magnitude?

Accepted Answer

A)  heats of fusion and deposition 
B)  heats of sublimation and condensation 
C)  heats of sublimation and deposition 
D)  heats of solidification and condensation 
A)  heats of fusion and deposition 
B)  heats of sublimation and condensation 
C)  heats of sublimation and deposition 
D)  heats of solidification and condensation

Question 10

Which of the following types of crystalline solids would be expected to have the lowest melting point?

Accepted Answer

A)  polar molecular 
B)  nonpolar molecular 
C)  macromolecular 
D)  ionic 
A)  polar molecular 
B)  nonpolar molecular 
C)  macromolecular 
D)  ionic

Question 11

Which is not characteristic of liquids?

Accepted Answer

A)  Collisions between particles occur often. 
B)  Particles are essentially independent of one another. 
C)  Under normal pressures, the particles are relatively close together. 
D)  The particles are not very compressible when pressure is applied. 
A)  Collisions between particles occur often. 
B)  Particles are essentially independent of one another. 
C)  Under normal pressures, the particles are relatively close together. 
D)  The particles are not very compressible when pressure is applied.

Question 12

How much heat energy in Joules is required to heat 16.0 g of copper from 23.0 °C to 66.1 °C? Specific heat of Cu = 0.382 J/(g °C)

Accepted Answer

A)  263 J 
B)  812 J 
C)  450 J 
D)  109 J 
A)  263 J 
B)  812 J 
C)  450 J 
D)  109 J

Question 13

How much heat must be absorbed to evaporate 14 g of NH3 from liquid to gas state at ?33 °C (condensation point)? Heat of condensation for NH3 = 1380 J/g

Accepted Answer

A)  19,000 J 
B)  91,000 J 
C)  46,000 J 
D)  62,000 J 
A)  19,000 J 
B)  91,000 J 
C)  46,000 J 
D)  62,000 J

Question 14

Which of the following quantities is needed in calculating the amount of heat energy released as water turns to ice at 0 °C?

Accepted Answer

A)  the mass and heat of solidification 
B)  heat of fusion for water and the mass 
C)  heat of vaporization for water and the mass 
D)  heat of condensation for water and the mass 
A)  the mass and heat of solidification 
B)  heat of fusion for water and the mass 
C)  heat of vaporization for water and the mass 
D)  heat of condensation for water and the mass

Question 15

The vapor pressure of SnCl4 reaches 400 mm Hg at 92 °C, the vapor pressure of SnI4 reaches 400 mm Hg at 315 °C, the vapor pressure of PBr3 reaches 400 mm Hg at 150 °C, and the vapor pressure of PCl3 reaches 400 mm Hg at 57 °C. At 175 °C which substance would have the lowest vapor pressure?

Accepted Answer

A)  PBr3 
B)  SnI4 
C)  SnCl4 
D)  PCl3 
A)  PBr3 
B)  SnI4 
C)  SnCl4 
D)  PCl3

Question 16

Which of the following would be correct units for a heat of condensation value?

Accepted Answer

A)  J/°C 
B)  Cal/°C 
C)  g/°C 
D)  Cal/g 
A)  J/°C 
B)  Cal/°C 
C)  g/°C 
D)  Cal/g

Question 17

In a liquid sample of NCl3, what is the dominant intermolecular force present?

Accepted Answer

A)  London forces 
B)  hydrogen bonding 
C)  instantaneous bonding 
D)  dipole-dipole interactions 
A)  London forces 
B)  hydrogen bonding 
C)  instantaneous bonding 
D)  dipole-dipole interactions

Question 18

A sample of aluminum absorbed 9.86 J of heat and the temperature increased from 23.2 °C to 30.5 °C. What is mass of the aluminum? The specific heat of aluminum is 0.90 J/g °C.

Accepted Answer

A)  72 g 
B)  1.5 g 
C)  65 g 
D)  8.1 g 
A)  72 g 
B)  1.5 g 
C)  65 g 
D)  8.1 g

Question 19

Which of the following substances would be expected to have the highest boiling point?

Accepted Answer

A)  a nonpolar liquid 
B)  a polar liquid with hydrogen bonding 
C)  a polar liquid with weak dipole-dipole interactions 
D)  a nonvolatile liquid 
A)  a nonpolar liquid 
B)  a polar liquid with hydrogen bonding 
C)  a polar liquid with weak dipole-dipole interactions 
D)  a nonvolatile liquid

Question 20

Calculate the mass of gold (0.130 J/g °C) that requires 468 J to heat the metal from 21.6 °C to 33.2 °C?

Accepted Answer

A)  56.9 g 
B)  622 g 
C)  538 g 
D)  310 g 
A)  56.9 g 
B)  622 g 
C)  538 g 
D)  310 g

In the solid state disruptive forces are ________.

What is the heat of vaporization in J/g of an unknown liquid if 6823 J of heat are required to vaporize 58.0 g of the unknown at its boiling point?

Which of the following pairs of quantities is needed in calculating the amount of heat energy needed to change liquid water at 75 °C to steam at 110 °C?

How much heat energy is needed to convert 10.0 g of ice at ?10 °C to liquid water at 10 °C? Specific heat of ice = 2.09 J/(g°C) Heat of fusion of ice = 334 J/g Specific heat of water = 4.18 J/g°C

Use a dashed line to illustrate hydrogen bonding between a methanol molecule and a hydrogen fluoride molecule.

Gases are highly compressible because the particles ________.

A nonvolatile liquid would ________.

How much energy is required to change 12.9 g of solid Cu to molten Cu at 1083 °C (melting point)? Heat of fusion for Cu = 205 J/g

Which of the following would have the same numerical magnitude?

Which of the following types of crystalline solids would be expected to have the lowest melting point?

Which is not characteristic of liquids?

How much heat energy in Joules is required to heat 16.0 g of copper from 23.0 °C to 66.1 °C? Specific heat of Cu = 0.382 J/(g °C)

How much heat must be absorbed to evaporate 14 g of NH₃ from liquid to gas state at ?33 °C (condensation point)? Heat of condensation for NH₃ = 1380 J/g

Which of the following quantities is needed in calculating the amount of heat energy released as water turns to ice at 0 °C?

Which of the following would be correct units for a heat of condensation value?

In a liquid sample of NCl₃, what is the dominant intermolecular force present?

A sample of aluminum absorbed 9.86 J of heat and the temperature increased from 23.2 °C to 30.5 °C. What is mass of the aluminum? The specific heat of aluminum is 0.90 J/g °C.

Which of the following substances would be expected to have the highest boiling point?

Calculate the mass of gold (0.130 J/g °C) that requires 468 J to heat the metal from 21.6 °C to 33.2 °C?

The Science of Chemistry

Numbers From Measurements

Unit Systems and Dimensional Analysis

Basic Concepts About Matter

Atoms, Molecules, Formulas, and Subatomic Particles

Electronic Structure and Chemical Periodicity

Chemical Bonds

Chemical Nomenclature

Chemical Calculations: the Mole Concept and Chemical Formulas

Chemical Calculations Involving Chemical Equations

Gas Laws

Solutions

Acids, Bases and Salts

Oxidation and Reduction

Reaction Rates and Chemical Equilibrium

Nuclear Chemistry

Filters

Exam 11: States of Matter

In the solid state disruptive forces are ________.

What is the heat of vaporization in J/g of an unknown liquid if 6823 J of heat are required to vaporize 58.0 g of the unknown at its boiling point?

Which of the following pairs of quantities is needed in calculating the amount of heat energy needed to change liquid water at 75 °C to steam at 110 °C?

How much heat energy is needed to convert 10.0 g of ice at ?10 °C to liquid water at 10 °C? Specific heat of ice = 2.09 J/(g°C) Heat of fusion of ice = 334 J/g Specific heat of water = 4.18 J/g°C

Use a dashed line to illustrate hydrogen bonding between a methanol molecule and a hydrogen fluoride molecule.

Gases are highly compressible because the particles ________.

A nonvolatile liquid would ________.

How much energy is required to change 12.9 g of solid Cu to molten Cu at 1083 °C (melting point)? Heat of fusion for Cu = 205 J/g

Which of the following would have the same numerical magnitude?

Which of the following types of crystalline solids would be expected to have the lowest melting point?

Which is not characteristic of liquids?

How much heat energy in Joules is required to heat 16.0 g of copper from 23.0 °C to 66.1 °C? Specific heat of Cu = 0.382 J/(g °C)

How much heat must be absorbed to evaporate 14 g of NH3 from liquid to gas state at ?33 °C (condensation point)? Heat of condensation for NH3 = 1380 J/g

Which of the following quantities is needed in calculating the amount of heat energy released as water turns to ice at 0 °C?

The vapor pressure of SnCl4 reaches 400 mm Hg at 92 °C, the vapor pressure of SnI4 reaches 400 mm Hg at 315 °C, the vapor pressure of PBr3 reaches 400 mm Hg at 150 °C, and the vapor pressure of PCl3 reaches 400 mm Hg at 57 °C. At 175 °C which substance would have the lowest vapor pressure?

Which of the following would be correct units for a heat of condensation value?

In a liquid sample of NCl3, what is the dominant intermolecular force present?

A sample of aluminum absorbed 9.86 J of heat and the temperature increased from 23.2 °C to 30.5 °C. What is mass of the aluminum? The specific heat of aluminum is 0.90 J/g °C.

Which of the following substances would be expected to have the highest boiling point?

Calculate the mass of gold (0.130 J/g °C) that requires 468 J to heat the metal from 21.6 °C to 33.2 °C?

The Science of Chemistry

Numbers From Measurements

Unit Systems and Dimensional Analysis

Basic Concepts About Matter

Atoms, Molecules, Formulas, and Subatomic Particles

Electronic Structure and Chemical Periodicity

Chemical Bonds

Chemical Nomenclature

Chemical Calculations: the Mole Concept and Chemical Formulas

Chemical Calculations Involving Chemical Equations

Gas Laws

Solutions

Acids, Bases and Salts

Oxidation and Reduction

Reaction Rates and Chemical Equilibrium

Nuclear Chemistry

Filters

How much heat must be absorbed to evaporate 14 g of NH₃ from liquid to gas state at ?33 °C (condensation point)? Heat of condensation for NH₃ = 1380 J/g

In a liquid sample of NCl₃, what is the dominant intermolecular force present?