Ch.5 | Full Test Bank – States of Matter Gases, Liquids, and

General, Organic, and Biochemistry, 10e (Denniston)

Chapter 5 States of Matter: Gases, Liquids, and Solids

1) Which statement concerning the three states of matter is FALSE?

A) Particles of a gas are well separated, have no regular arrangement, and move at high speeds.

B) Particles of a solid have low kinetic energy, and are held close together by strong attractive forces.

C) Particles of a liquid have a rigid, ordered arrangement due to the high speeds of the liquid particles.

D) Gases have low densities and high compressibility due to the large amount of space between gas particles.

E) Phase changes between the three states of matter are physical changes; no change in the identity or composition of the substance occurs.

2) Gas pressure is a result of which of the following?

A) collisions of gas particles with each other

B) expansion of gas particles in an open container

C) the resistance of gas particles to flow

D) collisions of gas particles with the walls of the container

E) compressibility of gas particles

3) Which of the following statements correctly describes Boyle's Law?

A) The volume of a gas is directly proportional to the number of moles of the gas, if the pressure and temperature remain constant.

B) The volume of a gas is directly proportional to the Kelvin temperature of the gas, if the pressure and amount of gas remain constant.

C) The pressure of a gas is inversely proportional to the volume of the gas, if the temperature and amount of gas remain constant.

D) The pressure of a gas is directly proportional to the Kelvin temperature of the gas, if the volume and amount of gas remain constant.

E) The total pressure exerted by a mixture of gases in a container is the sum of the partial pressures that each gas would exert alone.

4) Which of the following statements correctly describes Charles's Law?

A) The volume of a gas is directly proportional to the number of moles of the gas, if the pressure and temperature remain constant.

B) The volume of a gas is directly proportional to the Kelvin temperature of the gas, if the pressure and amount of gas remain constant.

C) The pressure of a gas is inversely proportional to the volume of the gas, if the temperature and amount of gas remain constant.

D) The pressure of a gas is directly proportional to the Kelvin temperature of the gas, if the volume and amount of gas remain constant.

E) The total pressure exerted by a mixture of gases in a container is the sum of the partial pressures that each gas would exert alone.

5) Which of the following statements correctly describes Avogadro's Law?

A) Equal volumes of any ideal gas contain the same number of moles, if measured at the same temperature and pressure.

B) The volume of a gas is directly proportional to the Kelvin temperature of the gas, if the pressure and amount of gas remain constant.

C) The pressure of a gas is inversely proportional to the volume of the gas, if the temperature and amount of gas remain constant.

D) The pressure of a gas is directly proportional to the Kelvin temperature of the gas, if the volume and amount of gas remain constant.

E) The total pressure exerted by a mixture of gases in a container is the sum of the partial pressures that each gas would exert alone.

6) Which of the following represent STP (Standard Temperature and Pressure) conditions?

A) T = 0 K and P = 1 atm

B) T = 273 K and P = 0 atm

C) T = 1 K and P = 1 atm

D) T = 273 K and P = 1 atm

E) T = 0°C and P = 760 atm

7) Dalton's Law of Partial Pressures states which of the following?

A) The total pressure exerted by a mixture of gases in a container is equal to the highest partial pressure exerted by any of the gases in the container.

B) The total pressure exerted by a mixture of gases in a container is the sum of the pressures that each gas would exert if present alone under similar conditions.

C) The total pressure exerted by a mixture of gases in a container is the average of the pressures that each gas would exert if present alone under similar conditions.

D) The total pressure exerted by a mixture of gases in a container is inversely proportional to the pressure that each gas would exert if present alone under similar conditions.

E) The total pressure exerted by a mixture of gases in a container is equal to the range of partial pressures of each gas in the container.

8) Which statement INCORRECTLY describes what happens to a sample of gas when it experiences an increase in temperature?

A) The volume of the gas increases, as long as the pressure remains constant.

B) The pressure of the gas increases, if the volume remains constant.

C) The kinetic energy of the gas particles increases.

D) The number of gas particles increases.

E) The gas particles move with increased speed.

9) Which gas under the specified conditions would come closest to exhibiting ideal gas behavior?

A) H2 at low pressure and high temperature

B) NH3 at low pressure and high temperature

C) H2 at high pressure and low temperature

D) NH3 at low pressure and low temperature

E) NH3 at high pressure and low temperature

10) At 100°C, which gas sample exerts the greatest pressure?

A) A

B) B

C) C

D) D

E) They would all exert the same pressure.

11) What process is responsible for the formation of dew on the grass early in the morning?

A) sublimation

B) evaporation

C) condensation

D) freezing

E) deposition

12) Two molecules of ethane experience what type of attractive forces?

A) London dispersion forces

B) dipole-dipole interactions

C) hydrogen bonding

D) ionic bonding

E) covalent bonding

13) Sarin is a nerve gas that was previously used as a chemical weapon. Considering the physical properties of sarin shown in the table, which statement about sarin is FALSE?

A) A sample of sarin at 0°C exists as a liquid.

B) A sample of sarin at room temperature (22°C) exists as a liquid.

C) A sample of sarin at -100°C exists as a solid.

D) A sample of sarin at 100°C exists as a gas.

E) A sample of sarin at 170°C exists as a gas.

14) Which of the following is(are) NOT a type of crystalline solid?

A) covalent solid

B) molecular solid

C) amorphous solid

D) ionic solid

E) metallic solid

15) What state(s) of matter is most compressible?

A) solid

B) liquid

C) gas

D) solid and liquid

E) liquid and gas

16) Which of the following is NOT a unit for measuring pressure?

A) Pa

B) kJ

C) atm

D) mm Hg

E) torr

17) What law predicts the expansion of a balloon when helium is added?

A) Boyle's Law

B) Charles's Law

C) Avogadro's Law

D) Ideal Gas Law

E) None of the choices are correct.

18) Consider 1.00 L of air in a patient's lungs at 37.0°C and 1.00 atm pressure. What volume would this air occupy if it were at 25.0°C under a pressure of 5.00 × 102 atm (a typical pressure in a compressed air cylinder)?

A) 1.35 × 10-3 L

B) 480 L

C) 2.08 × 10-3 L

D) 1.92 × 10-3 L

E) 374 L

19) Calculate the density of nitrogen gas (N2) at STP, in g/L. [Molar mass: N2, 28.0 g/mol]

A) 0.645 g/L

B) 0.800 g/L

C) 1.25 g/L

D) 2.39 g/L

E) 3.58 g/L

20) What is the volume occupied by a mole of an ideal gas, if the pressure is 626 mmHg and the temperature is 25.0°C?

A) 29.7 L

B) 3.28 × 10-3 L

C) 2.49 L

D) 3.91 × 10-2 L

E) 5.66 L

21) A gas sample is prepared in which the components have the following partial pressures: nitrogen, 555 mmHg; oxygen, 149 mmHg; water vapor, 13 mmHg; argon, 7 mmHg. What is the total pressure of this mixture?

A) 760 mmHg

B) 724 mmHg

C) 1480 mmHg

D) 386 mmHg

E) 614 mmHg

22) What property of liquids explains the formation of spherical water droplets on green leaves?

A) viscosity

B) surface tension

C) adhesion

D) vapor pressure

E) None of the choices are correct.

23) How can pure water be made to boil at a temperature below 100°C?

A) increase the volume of water

B) decrease the volume of water

C) increase the pressure above 1 atm

D) decrease the pressure below 1 atm

E) Both decrease the volume of water and increase the pressure above 1 atm are correct.

24) To which elements must hydrogen be bonded in order to display hydrogen bonding?

A) fluorine

B) oxygen

C) nitrogen

D) All of the choices are correct.

E) Both oxygen and nitrogen are correct.

25) A barometer measures

A) the pressure of a gas sample in a container.

B) the difference in pressure between two gas samples.

C) the difference in pressure between a gas sample and atmospheric pressure.

D) atmospheric pressure.

E) the pressure of an ideal gas.

26) Which of the following statements concerning gases is FALSE?

A) Gases are made up of tiny atoms or molecules that are in constant, random motion.

B) Gases expand to fill the shape and volume of their container because the rapidly moving particles experience negligible attractive forces.

C) Gas pressure is the result of particles of a gas colliding with each other.

D) As the temperature of a gas increases, the kinetic energy of the particles increases.

E) Gases are highly compressible because most of the volume occupied by a gas is empty space.

27) One standard atmosphere of pressure (1 atm) is equivalent to what pressure expressed in units of mm Hg?

A) 14.7 mm Hg

B) 380 mm Hg

C) 760 mm Hg

D) 0.333 mm Hg

E) 30 mm Hg

28) Aircraft cabins are pressurized for passenger comfort and safety when cruising altitudes are greater than about 12,000 feet. If the inside of an aircraft cabin is pressurized to 10.9 psi, what is the equivalent pressure in atm?

A) 75 atm

B) 1.3 atm

C) 1.1 atm

D) 0.0009 atm

E) 0.74 atm

29) In the graph shown, which line is the best representation of Boyle's Law regarding behavior of a gas?

A) A

B) B

C) C

D) D

E) E

30) Who formulated the relationship between the volume and the pressure of a gas?

A) Boyle

B) Charles

C) Dalton

D) Gay-Lussac

E) Torricelli

31) A sample of oxygen occupies 1.00 L. If the temperature remains constant, and the pressure on the oxygen is decreased to one third the original pressure, what is the new volume?

A) 3.00 L

B) 1.50 L

C) 0.667 L

D) 0.500 L

E) 0.333 L

32) A given mass of oxygen at room temperature occupies a volume of 500.0 mL at 1.50 atm pressure. What pressure must be applied to compress the gas to a volume of only 150.0 mL?

A) 500 atm

B) 150 atm

C) 5.00 atm

D) 1.50 atm

E) 0.500 atm

33) A sample of oxygen gas occupies 3.0 L at a pressure of 1.5 atm. If the volume of this sample increases without changing the temperature or the amount of gas, what can be said about the pressure?

A) The pressure of oxygen will remain at 1.5 atm.

B) The pressure of oxygen will be less than 1.5 atm.

C) The pressure of oxygen will be greater than 1.5 atm.

D) The pressure of oxygen will be 4.5 atm.

E) It is impossible to predict.

34) A balloon filled with helium has a volume of 1.00 × 103 L at 20°C. What would be the balloon's volume at 30°C, if the pressure surrounding the balloon remains constant?

A) 6.7 × 102 L

B) 9.70 × 102 L

C) 1.03 × 103 L

D) 1.11 × 103 L

E) 1.50 × 103 L

35) Who discovered the gas law represented in the figure shown?

A) Boyle

B) Charles

C) Dalton

D) Avogadro

E) Torricelli

36) What is the volume occupied by one mole of helium at 0°C and 1 atm pressure?

A) 1.0 L

B) 22.4 L

C) 4.0 L

D) 40.0 L

E) 12.2 L

37) A helium-filled weather balloon is launched from the ground where the pressure is 752 mmHg and the temperature is 21°C. Under these conditions its volume is 75.0 L. When it has climbed to an altitude where the pressure is 89 mmHg and the temperature is 0°C, what is its volume?

A) 0.00 L

B) 8.24 L

C) 9.56 L

D) 588 L

E) 682 L

38) Hydrogen cyanide (HCN) is a poisonous gas that has been used to execute prisoners in the gas chamber. How many moles of HCN are present in a 67.0 L cylinder at 25.0°C that is registering a pressure of 742 mm Hg?

A) 2.24 mol

B) 2.67 mol

C) 2.81 mol

D) 31.9 mol

E) 1.71 × 103 mol

39) Carbon dioxide acts as a greenhouse gas by

A) absorbing visible radiation.

B) absorbing ultraviolet radiation.

C) absorbing infrared radiation.

D) storing solar energy.

E) trapping sunlight during photosynthesis.

40) Which of the following statements conflicts with the kinetic molecular theory of gases?

A) There are no forces between gas particles.

B) Gas particles occupy a negligible volume compared with the volume of their container.

C) The average kinetic energy of the gas particles is proportional to the absolute temperature.

D) Gas particles lose energy only when they collide with the walls of the container.

E) Gas particles are in constant, random motion.

41) What quantity is directly proportional to the kinetic energy of the particles in a gas?

A) distance between molecules

B) absolute temperature

C) atomic mass

D) formula mass

E) volume of the individual particles

42) Of the following gases, which will behave most like an ideal gas?

A) N2

B) HF

C) NH3

D) CH3Cl

E) CO

43) What is the experimental quantity that serves as a measure of resistance to flow of a liquid?

A) vapor pressure

B) surface tension

C) resistivity

D) viscosity

E) compressibility

44) An aerosol spray paint can with a volume of 350 mL registers a pressure of 4.5 atm at room temperature. What can be said about the pressure inside the can if it is stored outside during the winter months?

A) The pressure of the gas will be greater than 4.5 atm.

B) The pressure of the gas will be less than 4.5 atm.

C) The pressure of the gas will remain at 4.5 atm.

D) The pressure of the gas will be 1575 atm.

E) It is impossible to say anything about the pressure without additional information.

45) Surface tension

A) increases with increasing temperature.

B) is unaffected by temperature.

C) is higher for nonpolar substances than for polar ones.

D) is lowered by surfactants.

E) is the same as viscosity.

46) What is the term that describes a liquid changing to a vapor at a temperature less than its boiling point?

A) evaporation

B) sublimation

C) dissociation

D) condensation

E) supercooling

47) Which one of the following substances, with their structures shown, will NOT display hydrogen bonding?

A) A

B) B

C) C

D) D

E) E

48) How are the volume and temperature of a gas related?

A) They are directly related when the pressure and amount of gas remain constant.

B) They are inversely related when the pressure and amount of gas remain constant.

C) They are equal to each other when the pressure and amount of gas remain constant.

D) There is no apparent relation between the two.

E) The amount and type of gas must be specified in order to determine their relationship.

49) According to the kinetic molecular theory, which statement concerning gases is TRUE?

A) Gases are mostly empty space.

B) The average kinetic energy of the molecules increases with decreasing temperature.

C) Gas molecules are strongly attracted to each other.

D) When gas molecules collide they lose energy.

E) Gas molecules are very closely packed together.

50) A gas with pressure of 5.0 atm is compressed at constant temperature from 10.0 L to 2.0 L. What is the pressure of the gas after it is compressed?

A) 4.0 L

B) 1.0 × 102 L

C) 1.0 L

D) 0.40 L

E) 25 L

51) A balloon at 25°C has 1.00 L of air. The balloon is heated to 40°C at constant pressure. What is the new volume?

A) 1.00 × 103 L

B) 1.05 L

C) 1.60 L

D) 15.0 L

E) 2.25 L

52) A balloon containing helium at constant pressure and temperature has the volume doubled by adding a more helium. Which statement(s) is(are) TRUE?

A) The number of helium atoms doubled.

B) The number of moles of helium doubled.

C) The mass of helium in the balloon doubled.

D) All of the statements are true.

E) All of the statements are false.

53) What mass of helium is contained in a 2.0 L balloon at 30.0°C and 735 mm Hg?

A) 26.5 g

B) 0.477 g

C) 514 g

D) 66.1 g

E) 0.312 g

54) Which of the following is a statement of Dalton's law of partial pressure?

A) The total pressure of a mixture of gases is the sum of the partial pressure of each gas that makes up the mixture.

B) The partial pressure of a gas is equal to the total pressure of the mixture.

C) Gases can exist as mixtures at STP only.

D) The total pressure of a mixture of gases is the product of the partial pressures of each gas in the mixture.

E) In a mixture of two gases, the pressure of each gas is 1/2 the total pressure.

55) Which statement is true concerning an ideal gas?

A) Gases behave more ideally at low temperatures than at high temperatures.

B) Polar molecules are more ideal than nonpolar molecules.

C) Gases behave more ideally at low pressure than at high pressure.

D) Both the statements Gases behave more ideally at low temperatures than at high temperatures and Polar molecules are more ideal than nonpolar molecules are correct.

E) Both the statements Polar molecules are more ideal than nonpolar molecules and Gases behave more ideally at low pressure than at high pressure are true.

56) Glycerol is a very polar compound. Dimethyl ether is only slightly polar. Which statement is TRUE?

A) Glycerol is less viscous than dimethyl ether.

B) Glycerol will have a greater surface tension than dimethyl ether.

C) Dimethyl ether has a lower vapor pressure than glycerol.

D) The viscosity of both substances will increase with increasing temperature.

E) Glycerol will evaporate at a faster rate than dimethyl ether.

57) Which of the following is TRUE for a liquid that is placed in a sealed container?

A) Evaporation of the liquid cannot occur.

B) Once equilibrium is established between the liquid and the vapor, the rate of the evaporation process will equal the rate of condensation.

C) All molecules stay in the liquid state.

D) Condensation of the evaporated molecules in the jar can only occur once all of the liquid molecules are in the vapor (or gaseous) state.

E) A set vapor pressure will be reached, which is the same at all temperatures.

58) Which substance is expected to have the highest boiling point?

A) CO2

B) HCl

C) CH3OH

D) CH4

E) BF3

59) Which statement about a crystalline solid is always TRUE?

A) A crystalline solid has a regular repeating structure of the atoms, ions, or molecules that make up the solid.

B) A crystalline solid will always have a high melting point.

C) A crystalline solid will always have a low melting point.

D) A crystalline solid contains only ionic bonds.

E) A crystalline solid is another name for an amorphous solid.

60) Which property is typical for molecular solids?

A) consist of only metal atoms

B) contain ionic and covalent bonds

C) have low melting points

D) have no organized structure

E) will boil at very high temperature

61) Liquids and solids are both highly compressible.

62) The density of hydrogen gas is lower than that of uranium hexafluoride (UF6) gas if both are measured at STP.

63) Dalton's Law states that the volume of a gas varies directly with the absolute temperature.

64) Ethylene glycol molecules have a greater attraction for cyclopentane molecules than for each other.

65) When acetone (a component of nail polish remover) evaporates, hydrogen bonds between acetone molecules must be broken up.

66) Polar gases exhibit more ideal behavior than nonpolar ones.

67) As temperature increases, viscosity decreases.

68) Glycerol has a lower viscosity than ethanol.

69) Detergents and soaps decrease the surface tension of water.

70) The boiling point of a liquid is dependent on the atmospheric pressure.

71) The temperature in which water boils inside a pressure cooker is lower than in an open pan at sea level.

72) Polar compounds generally have higher boiling points than nonpolar compounds of similar molecular weight.

73) All compounds containing both oxygen and hydrogen will exhibit hydrogen bonding.

74) Ionic compounds tend to have higher melting points than molecular compounds.

75) The attractive forces between acetone molecules are stronger than the attractive forces between water molecules.

76) Metals conduct electricity well due to the mobility of the metal ions in the solid.