Deck 6: Gases, Liquids, Solids, and Intermolecular Forces

Question 1

Matter is more likely to exist in the ________ state as the temperature is lowered.

A) solid
B) liquid
C) gaseous
D) elemental

Answer 1

solid

Question 2

Which state of matter is characterized by having molecules close together, but moving randomly?

A) gas
B) liquid
C) solid
D) all of these

Answer 2

liquid

Question 3

The temperature at which a solid melts is the melting point of the solid. The melting point is an indication of the intermolecular forces that hold a solid together. Aluminum melts at 660°C. Gold melts at 1064°C. Lead melts at 328°C. Which one of the following ranks the intermolecular forces in these solid elements from the strongest to the weakest?

A) Au > Al > Pb
B) Al > Au > Pb
C) Pb > Au > Al
D) Au > Pb > Al

Answer 3

Au > Al > Pb

Question 4

The process by which a liquid is converted to a gas is called

A) sublimation.
B) condensation.
C) melting.
D) vaporization.

Question 5

The temperature at which a liquid becomes a gas is called the

A) melting point.
B) boiling point.
C) sublimation point.
D) decomposition point.

Question 6

The temperature at which a liquid becomes a solid is called the

A) melting point.
B) decomposition point.
C) boiling point.
D) condensation point.

Question 7

The degree of order of matter is directly proportional to the cohesive forces that hold the matter together. In other words, the more organized the state of matter, the stronger the "glue" that holds it together. Which of the following ranks these cohesive forces from the state with the strongest to that with the weakest cohesive forces?

A) gas > liquid > solid
B) liquid > solid > gas
C) solid > liquid > gas
D) solid = gas = liquid

Question 8

The temperature at which a solid melts is the melting point of the solid. The melting point is an indication of the intermolecular forces that hold the solid together. Water melts at 0°C. Table sugar (sucrose) melts at 285°C. Gallium, Ga, melts at 30°C. Which one of the following ranks the intermolecular forces in these solids from the strongest to the weakest?

A) Ga > water > sucrose
B) sucrose > Ga > water
C) water > sucrose > Ga
D) Ga > sucrose > water

Question 9

Which of the following ranks the three states of matter from most to least ordered?

A) gas > liquid > solid
B) gas > solid > liquid
C) solid > gas > liquid
D) solid > liquid > gas

Question 10

Matter is more likely to exist in the ________ state as the temperature is raised.

A) solid
B) liquid
C) gas
D) elemental

Question 11

Which state of matter is characterized by having molecules close together and confined in their movement?

A) gas
B) liquid
C) solid
D) all of these

Question 12

The process by which a solid is converted to a gas is called

A) liquefaction.
B) vaporization.
C) sublimation.
D) condensation.

Question 13

List the disadvantage of using supercritical carbon dioxide.

A) Precision electrical parts are degreased.
B) Oils are isolated from the plant source.
C) Special equipment is needed for the high temperature and high pressure.
D) Coffee is decaffeinated.

Question 14

Matter is more likely to exist in the ________ state as the pressure is increased.

A) solid
B) liquid
C) gaseous
D) elemental

Question 15

Which state of matter is characterized by having molecules far apart and moving randomly?

A) gas
B) liquid
C) solid
D) all of these

Question 16

The process by which a gas is converted to a liquid is called

A) condensation.
B) ionization.
C) sublimation.
D) vaporization.

Question 17

The process by which a liquid is converted to a solid is called

A) condensation.
B) freezing.
C) liquefaction.
D) vaporization.

Question 18

The process by which a gas is converted to a liquid is called

A) condensation.
B) melting.
C) vaporization.
D) sublimation.

Question 19

The temperature at which a liquid boils is the boiling point of the liquid. The boiling point is an indication of the intermolecular forces that hold the matter in the liquid state. Water, H₂O, boils at 100°C. Ethanol, C₂H₆O boils at 78°C. Ammonia, NH₃, boils at -33°C. Which one of the following ranks the intermolecular forces in these liquids from the strongest to the weakest?

A) Water > Ammonia > Ethanol
B) Ammonia > Ethanol > Water
C) Ethanol > Water > Ammonia
D) Water > Ethanol > Ammonia

Question 20

Matter is more likely to exist in the ________ state as the pressure is reduced.

A) solid
B) liquid
C) gas
D) elemental

Question 21

Methanol

A) can dissolve in water and will not conduct electricity.
B) can dissolve in water and will conduct electricity.
C) does not dissolve in water and will not conduct electricity.
D) does not dissolve in water and will conduct electricity.

Question 22

The attraction between an ion and water molecules is

A) ion-ion interaction.
B) ion-dipole interaction.
C) hydrogen bonding.
D) dispersion interaction.

Question 23

When an ionic compound dissolves in water,

A) the negative ends of water molecules surround the negative ions.
B) the positive ends of water molecules surround the positive ions.
C) the negative ends of water molecules surround the positive ions.
D) the negative ends of water molecules surround both the negative and the positive ions.

Question 24

Methanol has the formula CH₃OH. What is the predominant intermolecular force between methanol molecules?

A) dipole forces
B) dispersion forces
C) hydrogen bonds
D) ionic bonds

Question 25

Which of the following properties are NOT a characteristic of ionic compounds?

A) They have low boiling points.
B) They are composed of a metal and a nonmetal.
C) They tend to be solids at room temperature.
D) They may be soluble in water.

Question 26

All of the following solvents are no longer widely used as solvents for nonpolar organic compounds EXCEPT

A) benzene.
B) methylene chloride.
C) supercritical carbon dioxide (scCO₂).
D) perchloroethylene.

Question 27

Water is a liquid at room temperature while methane is a gas. Which statement compares the intermolecular forces in these molecules correctly?

A) The intermolecular forces in methane are stronger than those in water.
B) The intermolecular forces in water are stronger than those in methane.
C) Both water and methane have the same intermolecular forces.
D) There is not enough information to compare these forces.

Question 28

Which of the following is the weakest?

A) dipole forces
B) dispersion forces
C) hydrogen bonds
D) ionic bonds

Question 29

Which of the following processes involves the removal of energy (heat)?

A) condensation
B) melting
C) sublimation
D) vaporization

Question 30

A gas

A) has a definite shape but no definite volume.
B) has a definite volume but no definite shape.
C) has both a definite shape and a definite volume.
D) has no definite shape and no definite volume.

Question 31

What is the predominant intermolecular force between HCl molecules?

A) ionic bonds
B) hydrogen bonds
C) dipole forces
D) dispersion forces

Question 32

A liquid

A) has a definite volume and a definite shape.
B) has a definite shape but no definite volume.
C) has a definite volume but no definite shape.
D) is readily compressible.

Question 33

What type of forces exist between bromine molecules in liquid bromine?

A) hydrogen bonding
B) dipole forces
C) dispersion forces
D) ionic bonds

Question 34

Ionic compounds have strong forces between particles. This means that generally ionic compounds are ________ at room temperature.

A) solids
B) liquids
C) gases
D) covalently bonded

Question 35

All of the following statements about scCO₂ are correct EXCEPT

A) It can dissolve substances, just as liquids can.
B) It flows rapidly, just as gases do.
C) It causes cancer.
D) It can make processes occur more rapidly.

Question 36

Which of the following compounds will have the highest melting point?

A) SO₂
B) BaF₂
C) N₂H₄
D) SCl₆

Question 37

Liquid hydrogen is used as one part of the booster fuel in the space shuttle. What type of forces exist between hydrogen molecules in liquid hydrogen?

A) hydrogen bonding
B) dipole forces
C) dispersion forces
D) ionic bonds

Question 38

Which of the following is NOT a property of an ionic compound? Ionic compounds generally

A) dissolve in water.
B) form solutions that conduct electricity well.
C) have melting points lower than those of molecular compounds.
D) require more energy to change from the liquid to the gaseous state.

Question 39

For which of the following is hydrogen bonding NOT a factor?

A) H₂O
B) NH₃
C) CI₄
D) CH₃OH

Question 40

Ethane has the formula CH₃CH₃. What is the predominant intermolecular force between ethane molecules?

A) dipole forces
B) dispersion forces
C) hydrogen bonds
D) ionic bonds

Question 41

The statement that the volume of a fixed amount of a gas at a constant pressure is directly proportional to its absolute temperature is known as ________ Law.

A) Charles's
B) Boyle's
C) Gay-Lussac's
D) Avogadro's

Question 42

In a solution, the solvent is

A) present in larger amount than the solute is.
B) dissolved in the solute.
C) always water.
D) always nonpolar.

Question 43

A balloon is inflated outdoors on a cold day in North Dakota at a temperature of -35°C to a volume of 3.0 L. The pressure remains constant. What is the volume of the balloon indoors at a temperature of 25°C?

A) 2.4 L
B) 3.8 L
C) 3.2 L
D) 2.1 L

Question 44

A gas is enclosed in a 10.0 L tank at 1200 mm Hg pressure. Which of the following is a reasonable value for the pressure when the gas is pumped into a 5.00 L vessel?

A) 2400 mm Hg
B) 600 mm Hg
C) 24 mm Hg
D) 42 mm Hg

Question 45

A gas is enclosed in a 15.0 L tank at 600 mm Hg pressure. Which of the following is a reasonable value for the pressure when the gas is pumped into a 3.00 L vessel?

A) 1000 mm Hg
B) 120 mm Hg
C) 3000 mm Hg
D) 1200 mm Hg

Question 46

At STP, 22.4 liters of nitrogen gas, N₂, will have a mass of

A) 14.0 g.
B) 22.4 g.
C) 28.0 g.
D) 35.0 g.

Question 47

Charles's Law relates the volume and temperature of a gas sample at constant pressure. What would be the temperature of a gas sample when its volume is 0 L?

A) 273°C
B) -273°C
C) 0°C
D) 273 K

Question 48

At STP, 1 mole of oxygen gas, O₂, will have a mass of

A) 16.0 g.
B) 22.4 g.
C) 28.0 g.
D) 32.0 g.

Question 49

At a given temperature and pressure, the volume of a gas is directly proportional to the amount of gas present. This is a statement of

A) Avogadro's Law.
B) Boyle's Law.
C) Charles's Law.
D) the Ideal Gas Law.

Question 50

A sample of gas at a temperature of 350 K has a volume of 4.00 L. The pressure remains constant. What is the volume of the gas at a temperature of 175 K?

A) 8.00 L
B) 6.50 L
C) 3.75 L
D) 2.00 L

Question 51

According to the kinetic-molecular theory, gas molecules have

A) strong interactions between molecules.
B) weak interactions between molecules.
C) little distance between molecules.
D) less energy than molecules of a solid.

Question 52

The pressure of a gas will increase when

A) the volume decreases.
B) the volume increases.
C) the temperature decreases.
D) the size of the container increases.

Question 53

The density of Xe at STP is

A) 5.86 g/L.
B) 16.4 g/L.
C) 32.8 g/L.
D) 48.2 g/L.

Question 54

A gas is enclosed in a cylinder fitted with a piston. The volume of the gas is 5.00 L at 0.500 atm pressure. The piston is moved to increase the volume to 3.00 L. Which of the following is a reasonable value for the pressure of the gas at the greater volume?

A) 0.300 atm
B) 0.833 atm
C) 30.0 atm
D) 0.0333 atm

Question 55

The density of O₂ gas at STP is

A) 0.714 g/L.
B) 1.00 g/L.
C) 1.43 g/L.
D) 1.69 g/L.

Question 56

Which of the following is NOT a postulate of the kinetic-molecular theory?

A) Molecules of a gas move rapidly and in straight lines.
B) The molecules in a gas are tiny compared to the distance between them.
C) The molecules of a gas are strongly attracted to each other.
D) If two molecules collide with each other, the total energy of the molecules before the collision is the same as their total energy after the collision.

Question 57

The volume of one mole of krypton at STP is

A) 12.4 liters.
B) 22.4 liters.
C) 12.4 gallons.
D) 6.02 × 10²³ liters.

Question 58

At STP, 22.4 liters of krypton gas, Kr, will have a mass of

A) 20.9 g.
B) 41.9 g.
C) 83.8 g.
D) 167 g.

Question 59

The kinetic-molecular theory of gases assumes which of the following?

A) There are weak but significant interactions between gas molecules.
B) The total amount of energy will change when gas molecules collide.
C) The average kinetic energy of gas molecules will increase when you lower the temperature of the gas.
D) Gas molecules move constantly and in straight lines.

Question 60

For a given amount of gas at a constant temperature, the volume of gas varies inversely with its pressure is a statement of ________ Law.

A) Charles's
B) Avogadro's
C) Boyle's
D) Curie's

Question 61

Assume that you have a sample of a gas. You know the volume, the temperature and the number of moles of the sample. Which of the following laws would you use if you wanted to calculate the pressure of the sample?

A) Boyle's Law
B) Charles's Law
C) Law of Combining Volumes
D) Ideal Gas Law

Question 62

In the ideal gas law equation, PV = nRT, R is known as

A) the pressure.
B) a radian.
C) the universal gas constant.
D) a revolution.

Question 63

A solution is a heterogeneous mixture.

Question 64

The phrase "like dissolves like" means that a polar substance will dissolve readily in a polar solvent.

Question 65

According to the kinetic-molecular theory, there is very little attraction between particles of a gas.

Question 66

Use the ideal gas law to calculate the volume occupied by 0.400 mol of nitrogen gas at 3.00 atm pressure and at 27°C. R = 0.0821 L _* atm/(K^*mol).

A) 3.28 L
B) 17.7 L
C) 0.296 L
D) 16.7 L

Question 67

Use the ideal gas law to calculate the temperature when 0.300 mol of nitrogen gas at 1.40 atm pressure occupies a volume of 11.2 L. R = 0.0821 L_* atm/(K^*mol).

A) 490 K
B) 637 K
C) 780 K
D) 157 K

Question 68

Melting is the change from the ________ state to the ________ state.

Question 69

If the temperature of a gas is lowered, the gas molecules will strike the walls of its container more frequently. (Assume that the container has a definite shape and volume.)

Question 70

A covalent bond is weaker than a hydrogen bond.

Question 71

Most organic solvents are toxic, but supercritical fluids are generally regarded as safe.

Question 72

Temperatures must be converted to the Celsius temperature scale when Charles's Law is used.

Question 73

Supercritical fluids require the use of special equipment to control the temperatures and high pressures needed for their use.

Question 74

It requires more energy to melt one mole of an ionic compound than one mole of a molecular compound.

Question 75

Supercritical water and scCO₂ are "generally regarded as safe" by the U.S. Food and Drug Administration and are often used in the food industry.

Question 76

If the pressure of a gas rises, the gas molecules will strike the walls of its container more frequently. (Assume that the container has a definite shape and volume.)

Question 77

Why are the melting points of ionic compounds higher than the melting points of molecular compounds?

Question 78

The conditions for standard temperature and pressure (STP) are 1 atm pressure and 0°C.

Question 79

Carbon dioxide is an example of a supercritical fluid.

Question 80

The ideal gas law can be used to determine a new volume for a gas when its temperature is changed.