Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

AP Chemistry > Chapter 6: the gaseous state > Flashcards

Chapter 6: the gaseous state Flashcards

1
Q

gases have similar .., which allows us to develop models to predict their …

A

physical behaviors; properties

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

a gas is a fluid with no definite … or fixed …

A

shape; volume

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

a gas fills the

A

total volume of its container

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

because a gas is mostly empty space, a gas is

A

compressible

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

the volume of a gas … when an external force is applied

A

decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

a liquid is a fluid with a

A

fixed volume but no definite shape

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

a liquid takes the …., but it does not…

A

shape of its container; expand to fill the container

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

a solid has both fixed … and …

A

shape; volume

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

liquids and solids are …

A

condensed phases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

condensed phases: phases that are resistant to … because the spaces between the particles are … and cannot ….

A

volume changes; small; readily change

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

because the individual particles in both the liquid and solid phases are …., but in the gas phase are …, the density of the gas phase is much … than the density of either of the condensed phases

A

closely packed; separated; lower

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

density is generally expressed in .. for a gas, but the densities of liquids and solids are expressed in …

A

grams per liter; grams per milliliter

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

when a gas under atmospheric conditions condenses to a solid or a liquid, the density increases by a fact of about

A

1000

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

liquids and solids are resistant to volume changes because the spaces between the particles are

A

small and cannot readily change

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

pressure is defined as the

A

force exerted on a surface divided by the area of the surface

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

the atmosphere exerts a pressure because of the

A

weight of the gas molecules in the air

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

a barometer measures the

A

pressure of the amosphere

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

gravitational attraction pulls down the column of mercury, leaving a … above it in the tube. the column stops falling when the pressure caused by the weight of the mercury is

A

vacuum; equal to the pressure exerted by the atmosphere

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

mercury level in barometer rises→

A

high pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

mercury level in barometer lowers→

A

low pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

mercury is used in barometers because it is a liquid with a

A

high density

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

a manometer measures pressure

A

differences

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

(manometer) the atmosphere exerts a … on the mercury surface at the open end of the tube, and the gas within the container exerts pressure on the …

A

pressure; other surface of the mercury

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

(manometer) the difference between the heights of the 2 mercury surfaces corresponds to the difference between the

A

gas pressure in the container and the atmospheric pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

for a closed-end manometer the pressure of the gas is … to the difference between the heights of the …

A

equal; two mercury surfaces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

si unit for pressure

A

pascal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

1 pa = 1 N/ m^2 =

A

1 kg/ m * s^2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

1 bar =

A

10^5 Pa

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

1 atm= … mm Hg

A

760

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

1 torr = … Pa

A

133.3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

1 atm= … torr

A

760

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

1 atm= … psi

A

14.7

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

psi is

A

pounds per square inch

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

1 atm= … kPa

A

101.325

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

1 atm= … bar

A

1.01325

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

1 atm= …. in Hg

A

29.92

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

the physical properties of all gases behave in the …, regardless of the …

A

same general manner; identity of the gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

4 independent properties that define the physical state of a gas:

A

pressure; volume; temperature; number of moles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

gas laws express the relationships between the

A

4 independent properties of gases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

volume of a gas increases as pressure

A

decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

boyle’s law states that at constant …, the … of a sample of gas is … proportional to the …

A

temperature; volume; inversely; pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

V=

A

constant X 1/P

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

PV=

A

constant

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
44
Q

P1V1=

A

P2V2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
45
Q

doubling the temperature causes the volume of the gas to

A

double

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
46
Q

charles’s law states that at constant …, the … of a fixed amount of gas is … to the absolute …

A

pressure; volume; directly proportional; temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
47
Q

V = (charles’s law)

A

constant * T

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
48
Q

at absolute zero the volume of the gas must be

A

zero

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
49
Q

at absolute zero the volume of gas is zero because all gases …. before they reach this temperature

A

condense to liquid/solid phase

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
50
Q

absolute zero: … degrees C; … K

A

-273.15; 0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
51
Q

V/T =

A

constant

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
52
Q

V1/T1=

A

V2/T2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
53
Q

avogadro proposed that at thes ame temperature and pressure, equal volumes of gases contain the

A

same number of particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
54
Q

avogadro;s law states that at constant pressure and temperature, the volume of a gas sample is …

A

proportional to the number of moles of gas present

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
55
Q

(avogadro’s law) V=

A

constant * n

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
56
Q

V1/n1 =

A

V2/n2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
57
Q

combined gas law:

A

P1V1/n1 = P2V2/n2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
58
Q

temps must be expressed in

A

kelvins

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
59
Q

R with units Latm/ molK

A

0.08206

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
60
Q

R with units kgm^2/s^2mol*K

A

8.314

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
61
Q

R with units J/mol*K

A

8.314

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
62
Q

R with units cal/mol*K

A

1.987

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
63
Q

SCUBA:

A

self-contained underwater breathing apparatus

64
Q

high pressures caused by water at depths greater than … starts to force more nitrogen gas to …. leading to a state of motor function loss, decision making inability, and impairment in judgment known as …

A

50 m; dissolve into the bloodstream and other tissues; nitrogen narcosis

65
Q

the bends: a diver ascends toward the surface too quickly and nitrogen …. which then collect in the … causing extreme pain and the body …

A

bubbles come out of the body tissues; joints; curls up

66
Q

reaction in air bags

A

decomposition of sodium azide

67
Q

divers use an air mix that contains a lot of … gas, because helium doesn’t …

A

helium; dissolve in body tissues to a large extent

68
Q

divers can also use air mixes that contain …, but this can cause …, which thus results in uncontrollable …

A

heliox; high-pressure nervous syndrome; shaking

69
Q

trimix: mixture of … o2, … n2, and … He

A

10%; 20%; 70%

70
Q

ideal gas law:

A

PV=nRT

71
Q

R is the

A

ideal gas constant

72
Q

the value of the constant R is determined

A

experimentally

73
Q

measurements show that the volume of 1 mol of an ideal gas at standard temperature and pressure is

A

22.41 L

74
Q

standard temperature and pressure:

A

1 atm; 0 degrees C/273K

75
Q

the ideal gas law expresses the interrelationships of

A

volume, pressure, amount, and temperature

76
Q

we use the term ideal because under certain conditions the behavior of gases

A

deviates from that predicted by the ideal gas law

77
Q

the idea gas law is used to determine the value of any of the four properties–…., given values of the other three

A

pressure, volume, amount, and temperature of a gas

78
Q

before the development of mass spectrometry, the molar masses of many substances were determined by using the

A

ideal gas law

79
Q

the … of any given gas under a fixed set of conditions is also calculated from the ideal gas law

A

density

80
Q

at constant pressure and temperature, the density of a gas is directly related to its

A

molar mass

81
Q

just as in solution, reacting species in the gas phase can readily …, a necessary requireent for reactions to occur

A

collide

82
Q

use the ideal gas law to convert the moles of a gas sample to its

A

equivalent volume

83
Q

in chemical reactions at constant temp and pressure, the volumes of gases combine in the

A

same proportions as the coefficients of the equation

84
Q

we can directly calculate the volume of a gas produced b a reaction of gases in a chemical reaction, as long as the

A

pressure and temperaure of the gases are the same

85
Q

we do not need a pue sample of gas to use the

A

ideal gas law

86
Q

many of the early experiments that led to the formulation of the gas laws were performed with samples of

A

air rather than pure substances

87
Q

In 1801, English scientist John dalton realized that each gas in a mixture of gases exerts a pressure, called a …, which is the same as if the gas…

A

Partial pressure; occupied the container by itself

88
Q

Dalton’s law of partial pressure:

A

Pt = Pa + Pb

89
Q

A mixture of gases is a

A

Solution

90
Q

A convenient concentration unit to describe this gaseous mixture is the

A

Mole fraction

91
Q

Mole fraction: the number of moles of one component of a mixture divided by

A

The total number of moles of all substances present in the mixture

92
Q

χa =

A

Moles of component A/ total moles of all substances

93
Q

χa=

A

nA/ ntotal

94
Q

χa+χb+χc+….+χn=

A

1

95
Q

Pa =

A

χa x Pt

96
Q

chemists measure the volume of a gas generated in a reaction by

A

determining the volume of water displaced

97
Q

the gas sample collected by displacement of water is not pure, because some

A

water molecules are also present in the gas phase

98
Q

the partial pressure of water present in the gas phase depends on the

A

temperature of the water

99
Q

to determine the partial pressure of the gas collected, you must subtract the partial pressure of the water vapor from the

A

total pressure

100
Q

scientists made measurements of volumes and temperatures of gases to show that the volume of a gas at constant pressure is

A

proportional to its temperature in kelvins

101
Q

chemists sought to understand why a single law can describe the physical behavior of

A

all gases, regardless of the nature/size of the gas particles

102
Q

kinetic molecular theory describes the

A

behavior of gas particles at the molecular level

103
Q

(4 postulates of kinetic theory) a gas consists of … that are in … and …. no …. exist between any two gas particles

A

small particles; constant; random motion; forces of attraction or repulsion

104
Q

(4 postulates of kinetic theory) gas particles are very … compared with the ….

A

small; average distance that separates them

105
Q

(4 postulates of kinetic theory) collisions of gas particles with … and with the …. are …

A

each other; walls of the container; elastic

106
Q

(4 postulates of kinetic theory) elastic: no loss in … when …

A

total kinetic energy; particles collide

107
Q

(4 postulates of kinetic theory) the average kinetic energy of gas particles is proportional to the

A

temperature on the kelvin scale

108
Q

(kinetic molecular theory) the particles occupy only a small part of the ….; most of the … is …

A

volume of the container; volume; empty space

109
Q

(kinetic molecular theory) the gas particles are in

A

constant motion

110
Q

(kinetic molecular theory) the … and … of the particles change when they collide, but the … does not change

A

direction; speed; total energy of the gas

111
Q

(kinetic molecular theory) the energy of the gas changes only if the

A

temperature changes

112
Q

(kinetic molecular theory) the kinetic molecular theory assumes that the pressure exerted by a gas comes from the

A

collisions of the individual gas particles with the walls of the container

113
Q

(kinetic molecular theory) pressure increases if the … or …. increases, because both will increase the … on the wall

A

energy of the collisions; the number of wall collisions per second; force

114
Q

the kinetic molecular theory is consistent with the

A

ideal gas law

115
Q

as the size of a container decreases (at constant temperature), the number of … of the gas particles with the …. during any time interval …, because the particles have less … between collisions with the walls

A

collisions; walls per unit area; increases; distance to travel

116
Q

at constant temperature, the average force of each collision …, but in a smaller volume, the same number of particles strike a given area of the wall …, so the pressure of gas in the container …

A

does not change; more often; increases as volume decreases

117
Q

with an increase in temp and thus an increase in kinetic energy, each collision exerts a …, and the number of collisions per unit area per time …

A

greater force on the walls; increasese

118
Q

if pressure is to remain constant, the size of the container must …, reducing the number of these more …

A

increase; energetic collisions per unit area

119
Q

increasing the number of gas particles in a container increases the

A

number of collisions with the walls per unit area per unit time

120
Q

not all gas particles move at the same

A

speed

121
Q

the relationship of the average kinetic energy of the gas particles to the speed (u) of the particles is:

A

KE= 1/2mu^2

note: KE and u have lines over them, indicating that they are averages

122
Q

the square root of u^2 (u with a line over it) is called the …, labeled …, and is used to indicate the …

A

root-mean-square (rms) speed; urms; average speed of a gas

123
Q

from the mathematical treatment of the kinetic theory of gases, we can determine the

A

relative number of gas particles that have any particular speed

124
Q

root mean square speed is not the same as the

A

most probable speed (maximum of graph)

125
Q

plots that show speed and number of particles:

A

maxwell-boltzmann distribution curves

126
Q

if the temperature increases, the … increases, the curve …, and both the most probable speed and urms shift to …

A

average speed; broadens; greater values

127
Q

the average kinetic energy of the gas particles is proportional to the .., and kinetic molecular theory predicts that the rms speed is related to … and … by the equation:

A

temperature; temperature; molar mass;

urms=√(3RT)/M

128
Q

R in the urms calculation is

A

8.314 J/molK

129
Q

molar mass in urms is expressed n

A

kilograms per mole

130
Q

the rms speed of a gas sample is proportional to the square root of … and inverely proportion al to the square root of …

A

temperature; molar mass

131
Q

at constant temp, gases with greater maolar masses ave lower

A

rms speeds

132
Q

the observation that heavier particles have lower rms speeds is expected because the molecules in a heavier sample must move more … as thea verage kinetic energies of all gases are the .. at a given temperature

A

slowly; same

133
Q

diffusion is the

A

mixing of particles caused by motion

134
Q

the faster the molecular motion, the faster a gas

A

diffuses

135
Q

the rate of diffusion is always less than the …, because collisions prevent the particles from ..

A

rms speed of the gas; moving in a straight line

136
Q

effusion is the passage of a gas through

A

a small hole into an evacuated space

137
Q

graham’s law states that the rte of … of a gas is … to the square root of its …

A

effusion; inversely proportional; molar mass

138
Q

the kinetic molecular theory explains graham’s law because the rms speed of the gas particles is inversely proportional to the

A

square root of their molar mass

139
Q

rate of effusion of gas a/ rate of effusion of gas B =

A

√(molar mass of B/ molar mass of A)

140
Q

gases with greater rates of effusion escape through the hole in

A

shorter lengths of time

141
Q

the time it takes for a gas to effuse, t, is .. to the rate of effusion

A

inversely proportional

142
Q

most gases obey the ideal gas law quite closely at a pressure o about … and a temperature well above the … of the substance

A

1 atm; boiling point

143
Q

for a gas that follows the ideal gas law, the measured values of PV/nRT graph to a

A

straight line equalling 1

144
Q

as the pressure increases to high values, … occur

A

deviations

145
Q

deviations from the ideal gas law occur under extreme conditions because two of the assumptions of the kinetic molecular theory simply are nto correct when

A

gas particles are close together

146
Q

these assumptions are: that gas particles are …; that no … exist between gas particles

A

small compared with the distances separating them; attractive forces

147
Q

at high pressure, the volume occupied by the individual individual particles is no longer negligible coompared with the

A

volume of the gas sample

148
Q

when the particle’s size is no longer negligibl, the actual volume available for the gas particles to move is

A

reduced

149
Q

gas particles that are attracted to each other do not … as … as predicted, reducing he … below that predicted by the ideal gas law

A

strike the wall; hard; pressure

150
Q

as the pressure increases, he particles are forced …, making this attractive interaction more important because because more gas particles are …

A

closer together; close to the one about to hit the wall

151
Q

at very high pressures, the effect of molecular volume is greater than that of

A

the attractive forces

152
Q

a gas deviates from the ideal gas law at … and … near the … and at very high …

A

temperatures; pressures; condensation point; high pressures

153
Q

the ideal gas law can be modified to include the effects of

A

attractive forces and the volume occupied by the particles

154
Q

van der waals equation: nRT-

A

(P + an^2/V^2)(V-nb)

155
Q

n: number of

A

moles

156
Q

b: constant that depends on the

A

size of the gas particles

157
Q

a: constant related to the strength of the

A

attractive forces

AP Chemistry (24 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions