Deck 7: Gases, Liquids, and Solids

Question 1

Which cylinder at STP will contain the greatest mass of gas particles?

A)a 5.0-L cylinder of neon
B)a 5.0-L cylinder of helium
C)a 5.0-L cylinder of nitrogen
D)a 5.0-L cylinder of hydrogen
E)All of the cylinders above contain the same mass of gas particles.

Answer 1

C

Question 2

A scuba diver typically begins a dive with a compressed air tank at 2, 350 psi. What is this pressure expressed in units of Pa?

A)0.0232 Pa
B)3.09 Pa
C)2.38 × 10⁸ Pa
D)1.62 × 10⁷ Pa
E)45.5 Pa

Answer 2

D

Question 3

Consider the balanced reaction: Zn(s)+ 2 HCl(aq) $\rightarrow$ ZnCl₂(aq)+ H₂(g). What volume of H₂(g)at STP can be generated when 134 g of zinc reacts?

A)2.05 L
B)45.9 L
C)5.98 L
D)3.00 × 10³ L

Answer 3

45.9 L

Question 4

The temperature of a 0.750-L gas sample at 25 °C and 2.00 atm is changed to 250 °C. What is the final pressure of the system, at constant volume?

A)20.0 atm
B)0.200 atm
C)3.51 atm
D)0.427 atm

Question 5

A sample of gas contains four gases with the following partial pressures: He (113 mm Hg), Ne (184 mm Hg), Ar (35 mm Hg), and Xe (445 mm Hg). What is the total pressure of the sample?

A)777 mm Hg
B)760. mm Hg
C)445 mm Hg
D)332 mm Hg

Question 6

How many moles are contained in 5.33 L of O₂ at standard temperature and pressure?

A)5.33 mol of O₂
B)1.00 mol of O₂
C)0.238 mol of O₂
D)22.4 mol of O₂
E)4.20 mol of O₂

Question 7

A weather balloon contains 233 L of helium at 22 °C and 760. mm Hg. What is the volume of the balloon when it ascends to an altitude where the temperature is -54 °C and 511 mm Hg?

A)2.24 × 10⁷ L
B)467 L
C)116 L
D)257 L

Question 8

A balloon that contains 0.500 L of helium at 25 °C is cooled to 11 °C, at a constant pressure. What volume does the balloon now occupy?

A)0.22 L
B)1.1 L
C)0.477 L
D)0.525 L
E)0.500 L

Question 9

A scuba diver typically begins a dive with a compressed air tank at 2, 350 psi. What is this pressure expressed in units of atmospheres?

A)160. atm
B)2.35 atm
C)3.45 × 10⁴ atm
D)3.09 atm
E)45.5 atm

Question 10

A sample of neon gas has a volume of 5.0 mL at a pressure of 1.50 atm. What is the pressure exerted by the gas if the volume is increased to 30.0 mL, at constant temperature?

A)0.25 atm
B)9.0 atm
C)1.5 atm
D)0.21 atm
E)7.5 atm

Question 11

How many moles of gas are contained in a scuba diver's 12.6-L tank filled with 3422 psi of air at 25 °C?

A)1760 moles
B)2.10 × 10⁴ moles
C)120. moles
D)1430 moles

Question 12

A patient's systolic pressure is measured as 128 mm Hg. What is this pressure in units of atm?

A)128 atm
B)1.28 atm
C)0.168 atm
D)9.73 x 10⁴ atm
E)8.71 atm

Question 13

Which assumption is not part of the kinetic-molecular theory of gases?

A)A gas consists of particles that move randomly and rapidly.
B)The size of gas particles is small compared to the space between the particles.
C)Because the space between gas particles is large, gas particles exert no attractive forces on each other.
D)The kinetic energy of gas particles does not change with increasing temperature.
E)When gas particles collide with each other, they rebound and travel in new directions.

Question 14

A scuba diver typically begins a dive with a compressed air tank at 2, 350 psi. What is this pressure expressed in units of mm Hg?

A)160. mm Hg
B)3.09 mm Hg
C)1.21 × 10⁵ mm Hg
D)1.79 × 10⁶ mm Hg
E)45.5 mm Hg

Question 15

An aerosol can has a pressure of 1.86 atm. What is this pressure expressed in units of mm Hg?

A)1.86 mm Hg
B)1410 mm Hg
C)1860 mm Hg
D)0.00245 mm Hg

Question 16

A birthday balloon contains helium at a pressure of 815 torr. What is this pressure expressed in units of mm Hg?

A)815 mm Hg
B)1.07 mm Hg
C)0.815 mm Hg
D)6.19 × 10⁵ mm Hg

Question 17

A gas cylinder containing 6.38 mol of neon has a pressure of 491 mm Hg at 295 K. If 3.22 mol of helium is added to this cylinder, at constant temperature and volume, what will be the pressure in the cylinder?

A)9.73 mm Hg
B)739 mm Hg
C)1460 mm Hg
D)248 mm Hg

Question 18

A 54.2 L sample of gas at 115 K is heated to 345 K, at constant pressure. What volume does the gas now occupy?

A)2.15 × 10⁶ L
B)163 L
C)18.1 L
D)732 L

Question 19

Which gas law describes the relationship between the volume and temperature of a sample of gas at constant pressure?

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

Question 20

Which cylinder at STP will contain the greatest number of gas particles?

A)a 5.0-L cylinder of neon
B)a 5.0-L cylinder of helium
C)a 5.0-L cylinder of nitrogen
D)a 5.0-L cylinder of hydrogen
E)All of the cylinders above contain the same number of gas particles.

Question 21

What volume does 7.50 × 10²⁰ molecules of O₂ occupy at STP?

A)22.4 L
B)1.68 × 10²² L
C)0.0279 L
D)2.79 L

Question 22

Air pressure at the bottom of Death Valley, at 282 ft below sea level, is 776 mm Hg. What are the partial pressures of O₂ and N₂, which compose 21% and 78% of the atmosphere, respectively?

A)210 mm Hg O₂ and 780 mm Hg N₂
B)160 mm Hg O₂ and 610 mm Hg N₂
C)160 mm Hg O₂ and 590 mm Hg N₂
D)163 mm Hg O₂ and 613 mm Hg N₂

Question 23

When a sample of gas is compressed from 6.0 L to 2.0 L at a constant temperature, the pressure of the gas triples.

Question 24

The size of gas particles is large compared to the space between the particles.

Question 25

A sample of gas contains four gases (He, Ne, Ar, and Xe)with the following partial pressures: He (43 mm Hg), Ar (835 mm Hg), and Xe (111 mm Hg). If the total pressure in the container is 1355 mm Hg, what is the partial pressure of Ne in the sample?

A)989 mm Hg
B)760. mm Hg
C)366 mm Hg
D)323 mm Hg

Question 26

Surface tension measures which of the following?

A)a liquid's resistance to flow
B)a liquid's resistance to spreading out
C)a liquid's ability to boil at low temperatures
D)the molecular weight of a compound

Question 27

Which is a molecular solid?

A)MgCl₂
B)Au
C)SiO₂
D)graphite
E)sucrose (C₁₂H₂₂O₁₁)

Question 28

Three of the four phase changes below are endothermic. Which phase change is NOT endothermic?

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

Question 29

An aerosol spray can with a volume of 350 mL registers a pressure of 4.5 atm at room temperature. What happens to the pressure of the gas inside the can if the can is stored outside during the winter months?

A)The pressure of the gas will remain at 4.5 atm.
B)The pressure of the gas will be greater than 4.5 atm.
C)The pressure of the gas will be less than 4.5 atm.
D)It is impossible to predict without knowing the amount of gas present inside the can.

Question 30

Whether a substance exists as a gas, liquid, or solid depends on the balance between the kinetic energy of its particles and the strength of the interactions between the particles.

Question 31

Atmospheric pressure in interstellar space is approximately 1 × 10^-17 torr at a temperature of -173 °C. How many gas molecules are present in 25, 000 L of interstellar space (about the volume of a bedroom)?

A)2 × 10⁷ molecules
B)4 × 10^-17 molecules
C)2 × 10¹⁰ molecules
D)3 × 10^-14 molecules

Question 32

Hydrogen peroxide decomposes to give water and oxygen gas according to the equation below. If 3.0 moles of hydrogen peroxide decompose, what volume of oxygen gas is produced at a pressure of 1.0 atm and a temperature of 23 °C? 2 H₂O₂(l) $\rightarrow$ 2 H₂O(l)+ O₂(g)

A)1.9 L of O₂
B)2.8 L of O₂
C)24 L of O₂
D)36 L of O₂
E)73 L of O₂

Question 33

Which is a network solid?

A)MgCl₂
B)Au
C)SiO₂
D)Na
E)sucrose (C₁₂H₂₂O₁₁)

Question 34

When a sample of gas is heated from 80. °C to 160. °C at a constant pressure, the volume of the gas doubles.

Question 35

What is the volume of 62.3 g of nitrogen gas at STP?

A)22.4 L
B)49.8 L
C)99.6 L
D)2.78 L

Question 36

Which molecule(s)exhibit London dispersion forces?

A)CH₄
B)CHCl₃
C)NF₃
D)HF
E)All of the molecules above exhibit London dispersion forces.

Question 37

The normal boiling point of a liquid is the temperature at which its vapor pressure equals which of the following?

A)1 mm Hg
B)760 mm Hg
C)the pressure above the liquid
D)the vapor pressure of water

Question 38

At rest, the volume of air in the lungs is 615 mL at 760 mm Hg. When the volume of the lungs expands during inhalation, what happens to the pressure inside the lungs?

A)The pressure inside the lungs decreases, which draws air into the lungs.
B)The pressure inside the lungs increases, which forces air inside the lungs.
C)The pressure inside the lungs remains constant, and air readily flows into the lungs.
D)The pressure inside the lungs cannot be determined if the weight of the person is unknown.

Question 39

Which molecule(s)exhibit hydrogen bonding?

A)CH₄
B)CHCl₃
C)NF₃
D)HF
E)All of the molecules above exhibit hydrogen bonding.

Question 40

Which gas sample contains the largest number of moles?

A)4.0 L of O₂ at 273 K and 530 mm Hg
B)4.5 L of N₂ at 298 K and 610 mm Hg
C)3.8 L of He at 250 K and 880 mm Hg
D)5.0 L Ar at 300 K and 710 mm Hg

Question 41

If two compounds have the same molecular formula they will have the same boiling point.

Question 42

The stronger the intermolecular forces, the lower the vapor pressure of a substance at a given temperature.

Question 43

Evaporation is an endothermic process.

Question 44

STP is defined as a pressure of exactly one atmosphere and a temperature of 25 °C.

Question 45

London dispersion forces are the strongest type of intermolecular forces.

Question 46

Viscosity is a measure of the resistance of a liquid to flow freely.

Question 47

The value of the universal gas constant, R, changes as a function of temperature.

Question 48

The density of a sample of gas increases if the temperature is increased but the pressure is held constant.

Question 49

It requires less heat to melt a 10-g sample of water than to vaporize a 10-g sample of water.

Question 50

When the volume of a sample of gas is doubled and the Kelvin temperature is cut in half, the pressure of a sample remains constant.

Question 51

A gas cylinder containing 3.88 mol of helium has a pressure of 549 mm Hg at 298 K. If 1.22 mol of neon is added to this cylinder, at constant temperature and volume, the pressure will rise to 1750 mm Hg.

Question 52

London dispersion forces are exhibited by all covalent compounds.

Question 53

All solids are crystalline solids.

Question 54

The numerical value of the universal gas constant, R, depends on its units.

Question 55

A 22.4 g sample of O₂ will occupy less than 22.4 L at STP.

Question 56

The higher the vapor pressure of a compound, the higher the boiling point of the compound.

Question 57

When the pressure and temperature are held constant, the volume of a gas is inversely proportional to the number of moles present.

Question 58

If the lungs of a child hold 0.11 mol of air in a volume of 2.8 L, then the lungs of an average female adult, with a volume is 4.6 L, can be expected to hold 0.18 mol of air.

Question 59

When the volume of a sample of gas is doubled and the Kelvin temperature is doubled, the pressure of a sample remains constant.

Question 60

Polypropylene, a typical plastic, is an example of an amorphous solid.

Question 61

The pressure of a gas is proportional to its Kelvin temperature at constant volume and number of moles. Therefore increasing the temperature increases the pressure.

Question 62

Freeze-drying removes water from foods by the process of sublimation.

Question 63

The kinetic energy of gas particles _____ with increasing temperature.

Question 64

London dispersion forces are also referred to as van der Waals forces.

Question 65

Given these vapor pressures at 20 °C: butane, 1, 650 mm Hg; acetaldehyde, 740 mm Hg, Freon-113, 284 mm Hg, the compound with the lowest boiling point is _____.

Question 66

Charles's law can be used to explain the dangerous condition for scuba divers called "the bends", which is caused by the formation of nitrogen gas bubbles in the bloodstream.

Question 67

The type(s)of intermolecular forces exhibited by hydrogen bromide molecules, HBr, is/are _____.

Question 68

_____ is the pressure exerted by gas molecules in equilibrium with the liquid phase.

Question 69

Graphite is an example of a _____ solid.

Question 70

Energy is released when a less organized state is converted to a more organized state.

Question 71

When 88.4 g of hydrogen gas is put in a 25.8-L container at 300. K, the pressure will be 83.7 atm.

Question 72

The physical change indicated below represents the _____ of ethanol (C₂H₅OH).
C₂H₅OH(g) $\rightarrow$ C₂H₅OH(l)

Question 73

_____ are due to momentary changes in electron density in a molecule.

Question 74

Sarin, a nerve gas once used as a chemical weapon, has a melting point of -56 °C and a boiling point of 158 °C. A sample of sarin at room temperature (22 °C)exists as a liquid.

Question 75

Condensation is the opposite of sublimation.

Question 76

The type(s)of intermolecular forces exhibited by methane molecules, CH₄, is/are _____.

Question 77

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

Question 78

Gay-Lussac's law relates the _____ and temperature of a gas sample at constant volume.

Question 79

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