Deck 8: Gases, liquids, and Solids

Question 1

Which transformation is condensation?

A)liquid → solid
B)liquid → gas
C)solid → liquid
D)solid → gas
E)gas → liquid

Answer 1

gas → liquid

Question 2

Which combination of characteristics is most likely to be associated with molecules having strong dipole-dipole interactions?
I.polar bond
II.asymmetric shape
III.relatively low boiling point
IV.large surface area

A)I and III
B)II and IV
C)I and II
D)III and IV
E)I,II,III,and IV

Answer 2

I and II

Question 3

Which process is endothermic?

A)Water condenses on the outside of a cold soda can.
B)The melted wax hardens after a candle is extinguished.
C)Water vapor forms ice crystals in the upper atmosphere.
D)Gasoline spilled on the ground evaporates very quickly.
E)none of the above

Answer 3

Gasoline spilled on the ground evaporates very quickly.

Question 4

Which process is exothermic?

A)gas → liquid
B)liquid → gas
C)solid → liquid
D)solid → gas
E)none of the above

Question 5

Which is the best description of hydrogen bonding?

A)the unique chemical bonds between hydrogen and any other atom in the same molecule
B)the association between hydrogen of one molecule and a region of another molecule which has become negative due to temporary shifts in electron density
C)the polarity associated with a bond between hydrogen and a small electronegative atom to which it is bonded
D)the association between a hydrogen atom which is somewhat positive because it is bonded to a small electronegative atom and an atom of O,N or F on another molecule
E)the temporary attraction between hydrogen atoms on different molecules resulting from shifts in electron density

Question 6

Which molecule will undergo only London dispersion forces when interacting with other molecules of the same kind?

A)HF
B)CH₂Cl₂
C)C₄H₁₀
D)NaC₂H₃O₂
E)C₂H₅OH

Question 7

Which pair of molecules has the strongest dipole-dipole interactions?

A)NH₃ and CH₄
B)NH₃ and NH₃
C)CH₄ and CH₄
D)CO₂ and CO₂
E)CO₂ and CH₄

Question 8

Which description best fits a solid?

A)definite shape and volume;strong intermolecular attractions
B)definite volume;shape of container;moderate intermolecular attractions
C)definite volume;shape of container;no intermolecular attractions
D)volume and shape of container;no intermolecular attractions
E)volume and shape of container;strong intermolecular attractions

Question 9

Which transformation is melting?

A)liquid → solid
B)liquid → gas
C)solid → liquid
D)solid → gas
E)gas → liquid

Question 10

In comparing gases with liquids,gases have ________ compressibility and ________ density.

A)greater;smaller
B)greater;greater
C)smaller;smaller
D)smaller;greater
E)none of the above

Question 11

Which transformation is evaporation?

A)liquid → solid
B)liquid → gas
C)solid → liquid
D)solid → gas
E)gas → solid

Question 12

Which description best fits a liquid?

A)definite shape and volume;strong intermolecular attractions
B)definite volume;shape of container;moderate intermolecular attractions
C)definite volume;shape of container;no intermolecular attractions
D)volume and shape of container;no intermolecular attractions
E)volume and shape of container;strong intermolecular attractions

Question 13

What are the strongest intermolecular forces between pentane (C₅H₁₂)molecules?

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

Question 14

Which transformation is freezing?

A)liquid → solid
B)liquid → gas
C)solid → liquid
D)solid → gas
E)gas → liquid

Question 15

Which transformation is sublimation?

A)liquid → solid
B)liquid → gas
C)solid → liquid
D)solid → gas
E)gas → liquid

Question 16

Which intermolecular force is characteristic of compounds with low molar mass,which are liquids at room temperature and have relatively high boiling points?

A)dipole-dipole forces
B)London forces
C)hydrogen bonds
D)ionic bonds
E)covalent bonds

Question 17

Which of the following cannot have hydrogen bonds?

A)H₂O
B)HCl
C)HF
D)CH₃NH₂
E)NH₃

Question 18

The process of sublimation is ________ and involves a(an)________ in entropy.

A)exothermic;increase
B)exothermic;decrease
C)endothermic;increase
D)endothermic;decrease
E)endothermic;no change

Question 19

Which description best fits a gas?

A)definite shape and volume;strong intermolecular attractions
B)definite volume;shape of container;moderate intermolecular attractions
C)definite volume;shape of container;weak intermolecular attractions
D)volume and shape of container;no intermolecular attractions
E)volume and shape of container;strong intermolecular attractions

Question 20

In comparing liquids and gases,liquids have ________ compressibility and ________ density.

A)smaller;smaller
B)smaller;greater
C)greater;smaller
D)greater;greater
E)none of the above

Question 21

What would be the new pressure if a 400 mL gas sample at 380 mm Hg is expanded to 800 mL with no change in temperature?

A)190 mm Hg
B)380 mm Hg
C)570 mm Hg
D)760 mm Hg
E)950 mm Hg

Question 22

Which of the assumptions of the kinetic-molecular theory best explains the observation that a balloon collapses when exposed to liquid nitrogen (which is much colder than a cold winter day!!)?

A)Gas molecules move at random with no attractive forces between them.
B)The velocity of gas molecules is proportional to their Kelvin temperature.
C)The amount of space occupied by a gas is much greater than the space occupied by the actual gas molecules.
D)In collisions with the walls of the container or with other molecules,energy is conserved.
E)Collisions with the walls of the container or with other molecules are elastic.

Question 23

Which represents the largest pressure?

A)one atmosphere
B)five pounds per square inch
C)one millimeter of mercury
D)five mm Hg
E)one hundred pascals

Question 24

Which is not a correct statement of Charles's Law?

A)For a gas sample at constant pressure,temperature and volume are inversely proportional.
B)volume α temperature
C)V/T = a constant
D)
=

E)none of the above

Question 25

Rank the following in increasing order of increasing boiling point:
N₂ CH₃CH₂OH CO₂ HCl

A)CH₃CH₂OH < HCl < N₂ < CO₂
B)HCl < CH₃CH₂OH < N₂ < CO₂
C)N₂ < CO₂ < HCl < CH₃CH₂OH
D)CH₃CH₂OH < HCl < CO₂ < N₂
E)N₂ < CO₂ < CH₃CH₂OH < HCl

Question 26

The barometric pressure given in the local weather report is reported as inHg.What is the pressure in mmHg if the weatherman says the current pressure today is 29.75 in Hg?

A)75.57 mmHg
B)755.7 mmHg
C)117.1 mmHg
D)945.0 mmHg
E)760.0 mmHg

Question 27

Which measurement represents the largest value of pressure?

A)0.750 atm
B)785 mm Hg
C)755 torr
D)22.0 psi
E)100 kPa

Question 28

Using the kinetic molecular theory,as the temperature of a gas rises the pressure will also increase because

A)the gas molecules collide more frequently with the wall of container.
B)the gas molecules collide less frequently with the wall of a container.
C)the gas molecules collide more energetically with the wall of the container.
D)both the gas molecules collide more frequently and more energetically with the wall of the container.

Question 29

Which is not a correct statement of Boyle's Law?

A)For a gas sample at constant temperature,pressure and volume are inversely proportional.
B)pressure α 1/volume
C)pressure × volume = a constant
D)P₁V₁ = P₂V₂
E)none of the above

Question 30

Which of the assumptions of the kinetic-molecular theory best explains the observation that a gas can be compressed?

A)Gas molecules move at random with no attractive forces between them.
B)The velocity of gas molecules is proportional to their Kelvin temperature.
C)The amount of space occupied by a gas is much greater than the space occupied by the actual gas molecules.
D)In collisions with the walls of the container or with other molecules,energy is conserved.
E)Collisions with the walls of the container or with other molecules are elastic.

Question 31

Arrange the following in order of increasing intermolecular forces:
N₂ CH₃CH₂OH CO₂ HCl

A)N₂ < CO₂ < HCl < CH₃CH₂OH
B)CH₃CH₂OH < HCl < N₂ < CO₂
C)CH₃CH₂OH < HCl < CO₂ < N₂
D)HCl < CH₃CH₂OH < N₂ < CO₂
E)N₂ < CO₂ < CH₃CH₂OH < HCl

Question 32

When the volume of a gas is plotted against the Celsius temperature while holding pressure and the number of moles constant,the x-intercept will occur at what temperature?

A)0°C
B)-273°C
C)the boiling point of the gas
D)the melting point of the gas
E)100°C

Question 33

Volume and pressure are ________ proportional.

A)directly
B)inversely
C)all of the above
D)none of the above

Question 34

Which assumption of Kinetic Molecular Theory is not followed when a real gas shows non-ideal behavior?

A)Gas molecules move at random with no attractive forces between them.
B)The velocity of gas molecules is proportional to their Kelvin temperature.
C)The amount of space occupied by a gas is much greater than the space occupied by the actual gas molecules.
D)In collisions with the walls of the container or with other molecules,energy is conserved.
E)Collisions with the walls of the container or with other molecules are elastic.

Question 35

Which of the assumptions of the kinetic-molecular theory best explains Dalton's law of partial pressures?

A)Gas molecules move at random with no attractive forces between them.
B)The velocity of gas molecules is proportional to their Kelvin temperature.
C)The amount of space occupied by a gas is much greater than the space occupied by the actual gas molecules.
D)In collisions with the walls of the container or with other molecules,energy is conserved.
E)Collisions with the walls of the container or with other molecules are elastic.

Question 36

Which measurement represents the smallest value of pressure?

A)0.750 atm
B)785 mm Hg
C)755 torr
D)22.0 psi
E)100 kPa

Question 37

What is the new volume of a balloon originally at 755 torr and 5.00 L is placed in a container in which the pressure is increased to 1.25 atm?

A)6.29 L
B)3.97 L
C)0.159 L
D)302 L
E)39.7 L

Question 38

Most gases show variations from ideality at ________ pressure and ________ temperature.

A)high;low
B)low;high
C)high;high
D)low;low
E)moderate;moderate

Question 39

Sketch a graph illustrating Boyle's Law.Use a gas sample with a volume of 2.0 L at 0.75 atm and 25°C,and show at least two other points.

Question 40

The number of mm Hg in one atmosphere is

A)14.7.
B)760.
C)1.00.
D)29.9.
E)101.325.

Question 41

A sample of helium has a volume of 480 mL at 47.0°C and 740 mm Hg.The temperature is lowered to 22.0°C and the pressure to 625 mm Hg.What is the new volume?

A)266 mL
B)373 mL
C)524 mL
D)616 mL
E)1214 mL

Question 42

A balloon originally had a volume of 4.39 L at 44°C and a pressure of 729 torr.To what temperature must the balloon be cooled to reduce its volume to 3.78 L if the pressure is constant?

A)38°C
B)0.0°C
C) 72.9 °C
D)273°C
E)237°C

Question 43

How will the volume of a fixed sample of gas change if the pressure is doubled and its Celsius temperature is halved?

A)The change cannot be determined without more specific information.
B)It will double.
C)It will decrease by a factor of 4.
D)It will decrease by a factor of 2.
E)It will remain constant.

Question 44

Which of the following is the definition of standard temperature and pressure?

A)273°C and 760 torr
B)298 K and 1 atm
C)273 K and 760 mm Hg
D)0 K and 1 atm

Question 45

For the following reaction,if 11.2 L of nitrogen are reacted to form NH₃ at STP,how many liters of hydrogen will be required to completely consume all of the nitrogen?
N₂ + 3H₂ → 2NH₃

A)16.8 L
B)11.2 L
C)7.4 L
D)33.6 L
E)6.1 L

Question 46

How will the volume of a fixed sample of gas change if its pressure is doubled and the Kelvin temperature is doubled?

A)The change cannot be determined without more specific information.
B)It will double.
C)It will increase by a factor of 4.
D)It will decrease by a factor of 2.
E)It will not change.

Question 47

A sealed container with gas at 2.00 atm is heated from 20.0 K to 40.0 K.The new pressure is

A)0.500 atm.
B)1.00 atm.
C)4.00 atm.
D)2.14 atm.
E)1.87 atm.

Question 48

If the temperature of a 1.75 liter sample of gas is changed from 30.0°C to 20.0°C at constant pressure,what will be the new volume?

A)1.17 L
B)1.57 L
C)1.69 L
D)1.81 L
E)2.63 L

Question 49

A 250.mL sample of gas at 1.00 atm and 20.0°C has the temperature increased to 40.0°C and the volume increased to 500.mL.What is the new pressure?

A)0.374 atm
B)0.468 atm
C)0.534 atm
D)1.87 atm
E)2.14 atm

Question 50

According to Avogadro's Law,the volume of a gas will ________ as the ________ is increased while the ________ are held constant.

A)increase;number of moles;pressure and temperature
B)decrease;number of moles;pressure and temperature
C)increase;temperature;pressure and number of moles
D)decrease;pressure;temperature and number of moles
E)increase;pressure;temperature and number of moles

Question 51

What will be the new volume when 128 mL of gas at 20.0°C is heated to 40.0°C while pressure remains unchanged?

A)64.0 mL
B)120.mL
C)128 mL
D)137 mL
E)256 mL

Question 52

Which is a correct statement of Gay-Lussac's Law describing the behavior of a fixed amount of gas?

A)As pressure increases,volume increases at constant temperature.
B)As pressure increases,volume decreases at constant temperature.
C)As temperature increases,pressure decreases at constant volume.
D)As temperature increases,pressure increases at constant volume.
E)As temperature increases,volume increases at constant pressure.

Question 53

Chlorine gas is widely used to purify municipal water supplies and to treat swimming pool waters.Suppose that the volume of a particular sample of Cl₂ is 718 mL at 675 mmHg and 48°C,at what temperature (in °C)will the volume be 2.00 L if the pressure is 159 kPa?

A)1308°C
B)273°C
C)237°C
D)1581°C
E)-36.6°C

Question 54

How many moles of gas are present in a 10.0 liter sample at STP?

A)224 moles
B)22.4 moles
C)10.0 moles
D)2.24 moles
E)0.446 moles

Question 55

A sample of gas has a volume of 135 mL at 0.600 atm.What would be the volume if the pressure is decreased to 0.200 atm while temperature is held constant?

A)45.0 mL
B)101 mL
C)135 mL
D)180 mL
E)405 mL

Question 56

Sketch a graph illustrating Charles's Law.Use a gas sample with a volume of 2.0 L at 0.75 atm and 27°C,and show at least two other points.

Question 57

Consider a sample of helium and a sample of neon,both at 30.0°C and 1.5 atm.Both samples have a volume of 5.0 liters.Which statement concerning these samples is not true?

A)Each sample contains the same number of atoms of gas.
B)Each sample weighs the same amount.
C)Each sample contains the same number of moles of gas.
D)The density of the neon is greater than the density of the helium.
E)none of the above

Question 58

How many grams of N₂ are contained in an 11.2 liter sample at STP?

A)7.00
B)11.2
C)14.0
D)28.0
E)6.02 × 10²³

Question 59

How many grams of O₂ are contained in a 25.0 L sample at 5.20 atm and 28.0°C?

A)1810 g
B)168 g
C)84.2 g
D)5.26 g
E)0.164 g

Question 60

A 65 mL sample of argon gas has a temperature of 325°C.What will the temperature be in °C when the volume of the gas is decreased to 25 mL at constant pressure?

A)65°C
B)125°C
C)-43°C
D)1280°C
E)641°C

Question 61

The amount of energy involved in melting a substance without changing its temperature is called the

A)heat of vaporization.
B)calorie.
C)joule.
D)heat of fusion.
E)heat of combustion.

Question 62

The total pressure of a mixture of gases is

A)obtained by multiplying the individual pressures by the number of moles and averaging.
B)the sum of the partial pressures of the components.
C)dependent only upon the pressure of the gas which is present to the greatest extent.
D)the product of the individual pressures.
E)none of these

Question 63

What is the pressure in a 1.00 liter container of methane,CH₄,that contains 40.0 g of the gas at 25.0°C?

A)5.13 atm
B)61.0 atm
C)82.1 atm
D)979 atm
E)3920 atm

Question 64

At a high altitude water boils at 95°C instead of 100°C as at sea level because the

A)atmospheric pressure is greater.
B)atmospheric pressure is less.
C)climate is cooler.
D)vapor pressure of water is greater.
E)vapor pressure of water is less.

Question 65

In a gas mixture of 35% He and 65% O₂ the total pressure is 800 mm Hg.What is the partial pressure of O₂?

A)35 mm Hg
B)65 mm Hg
C)100 mm Hg
D)280 mm Hg
E)520 mm Hg

Question 66

What volume will be occupied by 8.00 g of oxygen,O₂,at STP?

A)5.60 L
B)11.2 L
C)22.4 L
D)13.4 L
E)4.00 L

Question 67

If a 0.614 g sample of a gas maintains a pressure of 238 mm Hg when contained in a 1.0 L flask at 0.0°C,what is molar mass of the gas?

A)44 g/mol
B)120 g/mol
C)8.8 g/mol
D)22 g/mol
E)5 g/mol

Question 68

What is the total pressure of a mixture of He and H₂ if the partial pressures are 320 mm Hg and 800 mm Hg respectively?

A)40 mm Hg
B)60 mm Hg
C)320 mm Hg
D)480 mm Hg
E)1120 mm Hg

Question 69

Calculate the volume of a 3.50 mol sample of carbon dioxide at 30.0°C and 0.900 atm.

A)8.54 × 10^-4 L
B)2.20 L
C)9.58 L
D)96.7 L
E)421 L

Question 70

The amount of energy associated with changing a liquid into a gas is called the

A)heat of vaporization.
B)heat of fusion.
C)heat of combustion.
D)joule.
E)calorie.

Question 71

List the five types of solids and at least two physical properties of each.Explain how the interparticle forces in that solid determine the properties you listed.

Question 72

What is the total pressure of a gaseous mixture that contains three gases with partial pressures of 0.845 atm,120 torr,and 210 mm Hg?

A)1175 torr
B)972 torr
C)0.411 atm
D)331 torr

Question 73

As the temperature of a liquid is lowered,what happens to its vapor pressure?

A)Its vapor pressure drops.
B)Its vapor pressure rises.
C)The vapor pressure may rise or drop depending on the liquid.
D)Its vapor pressure is independent of temperature.
E)Its vapor pressure first rises then falls.

Question 74

A mixture of the gases N₂,O₂,and He has a total pressure of 760 mm Hg.If the partial pressure of N₂ is 90 mm Hg and of O₂ is 270 mm Hg,what is the partial pressure of He?

A)1120 mm Hg
B)760 mm Hg
C)400 mm Hg
D)360 mm Hg
E)120 mm Hg

Question 75

A solid compound which has no definite crystalline structure and a poorly defined melting point is referred to as a(an)________ solid.

A)ionic
B)molecular
C)network covalent
D)amorphous
E)metallic

Question 76

The vapor pressure of a liquid

A)decreases with increasing temperature.
B)is independent of temperature.
C)is equal to one atmosphere at the normal boiling point.
D)cannot be measured.

Question 77

Calculate the volume of 5.00 mol of helium at 120.°C and 1520 mm Hg.

A)323 liters
B)80.6 liters
C)0.106 liters
D)0.0324 liters
E)none of the above

Question 78

When a liquid sample is taken from sea level to a higher elevation,what happens to the external (atmospheric)pressure on the liquid and the boiling point of the liquid?

A)Both decrease.
B)Both increase.
C)Pressure goes down but boiling point goes up.
D)Pressure goes up but boiling point goes down.

Question 79

List and describe two unique properties of water.Discuss the intermolecular force that causes these unusual properties.

Question 80

A sample of CO₂ gas at 100.°C has a volume of 250.mL at 760.mm Hg.How many moles of CO₂ are present?

A)0.00816 mol
B)0.0304 mol
C)6.20 mol
D)8.16 mol
E)23.14 mol