Chapter 6: Gases Flashcards
1
Q
volume of a gas equal the volume of its BLANK
A
container
2
Q
gases have neither fixed BLANK nor BLANK
A
shape or volume
3
Q
all gases form BLANK mixtures
A
homogeneous
4
Q
describe level of interaction of gas molecules
A
gas molecules have little interaction, they are relatively far apart from each other
5
Q
formula for gas pressure
A
force dvided by area
6
Q
in a liquid, gases occupy how much of the space
A
70%
7
Q
what does STP stand for
A
Standard Atmospheric Pressure
8
Q
1 atm equals how many mmHg/Torr
A
760 mmHg and 760 Torr
9
Q
how are volume and pressue related in gas laws
A
inversely related
10
Q
what is Boyle’s Law
A
gas volume is inversely proportional to pressure
11
Q
Boyle’s law formula
A
V1P1=V2P2
12
Q
what is Charles’s Law
A
gas volume is directly proportional to Kelvin temperature
13
Q
Charles’s Law formula
A
V1/T1=V2/T2
14
Q
Avogadro’s Law
A
voume of gas is proportional to molar amount
15
Q
Avogadro’s Law formula
A
V1/n1=V2/n2
16
Q
what is the gas constant in IGL
A
r = .08206 Latm/molk
17
Q
IGL standard temperature for gas
A
t= 0° C
18
Q
standard pressure for gas IGL
A
P = 1 atm
19
Q
IGL for volume
A
Liters
20
Q
IGL unit for pressure
A
atm
21
Q
IGL unit for temperature
A
Kelvin
22
Q
what is molar volume of a gas in IGL
A
V = 22.414 L for 1 mole of an ideal gas at STP
23
Q
Dalton’s Law
A
total pressure of the gas mixture equals the sum of partial pressure of the individual gasses in the mixture
24
Q
Dalton’s Law formula
A
P(total) = P(A) + P(B) + P(C)…
25
IGL equation
PV = nRT
26
mole fraction equation
X(A) = P(A)/P(total)
27
what does KMT stand for
kinetic molecular theory
28
what is KMT
model that explains behavior of gases
29
In KMT, gas consists of particles in what kind of motion
constant, random motion
30
In KMT, the size of gas particles is BLANK compared to the size of container
the size is negligible
31
In KMT, the strength of intermolecular forces is BLANK
negligible
32
In KMT, the average KE of gas particles is directly proportional to what?
Kelving temperature
33
In KMT, all collisions of the gas particles are BLANK. What does this mean?
Alll collisions are elastic, meaning there is no loss of KE
34
A real gas will have properties most like an idea gas at what temperature and pressure?
high temperature and low pressure
35
real gases differ from idea gases in that...
real gases have volume and particles that interact and collide
36
speed at which a molecules is traveling depends on what two things?
speed depends on mass of the molecule and temperature
37
the lighter a gas particle, the BLANK the speed
faster the gase's speed
38
formula for rms speed
u = √3RT / √M
39
what is effusion
escape of gas through a tiny orifice into an evacuated chamber
40
what is Graham's Law of effusion
rate of effusion is inversely proportional to the square root of the molar mass
41
what is diffusion
the mixing of two gases, from higher concentration to lower concentration
42
what is effusion rate?
the faster the particles move, the more likely they are to pass through the effusion orifice
43
deviations from idea gas behavior are largest when pressure is BLANK and temperature is BLANK
when pressure is high and temperature is low
44
when pressure is high, size becomes BLANK
significant
45
when temperature is low, attractive forces become BLANK
significant
46
what does "n" equal?
amount of gas in moles
47
in a J-tube, the height of Hg is proportional to what?
the pressure of the gas
48
define molar volume
volume occupied by 1 mole of a substance at T=0° C / 273.15 K and P=1atm
49
define pressure
amount of force per unit area
50
relationship between concentration and pressure
direct relationship: lower concentration=lower pressure
51
what is pressure measured with
barometer
52
what is atmospheric pressure
average pressure at sea level
53
what do simple gas laws describe
relationship between P, V, T, and n
54
what does extrapolate mean
to extend
55
what did Charles quantify?
relationship between volume and temperature
56
what happens to speed of particles when temperature increases?
particles move faster
57
the molar volume of a gas of 22.414 L only applies at what?
standard temperature and pressure
58
density of a gas equals
molar mass divided by molar volume
59
formula for molar gas
molar mass = mass/moles
60
describe the interaction of molecules in an ideal gas
molecules in an IG do not interact
61
general gas law formula
P1V1/T1 = P2V2/T2
62
one mole of an ideal gas at STP has a volume of what?
22.414 L
63
according to KMT, when gas density is very low...
particles are far apart
64
the IGL are most valid when...
when particle density is very low
65
when particle density is very low...
the distance between particles is greater than the particle size
66
describe kinetic energy at high temperatures
kinetic energy or particles is much greater than the strength of intermolecular forces
67
what is assumed of gas particles when kinetic energy is very high
it is assumed that gas particles don't interact, other than random collisions
68
describe the distance of gas particles at low pressures
gas particles are far away from each other
69
when gas particles are far away from each other, what is assumed?
the size of gas particles is negligible
70
observations lead to what?
laws
71
what does kinetic molecule theory do for gas laws
KMT provides reasons behind the laws
72
what is a gas
collection of particles in constant motion
73
when particle size is negligibly small, what can be said of volume?
the particles don't occupy volume
74
average kinetic energy depends ONLY on what?
temperature of gas
75
Can the speed of a GIVEN molecule in a gas double at constant temperature? Explain your answer.
Yes. At any given instant, there are a range of values of molecular speeds in a sample of gas. Any single molecule can speed up or slow down as it collides with other molecules. The average velocity of all the molecules is constant at constant temperature.
76
Describe what happens to the average kinetic energy of ideal gas molecules when the pressure of the gas is increased by reducing the volume at constant temperature.
average kinetic energy with remain constant due to constant temperature
77
Describe what happens to the average kinetic energy of ideal gas molecules when the pressure of the gas is increased by increasing the temperature at constant volume.
Av. KE will increase because temperature increased
78
Describe what happens to the average kinetic energy of ideal gas molecules when the average velocity of the molecules is increased by a factor of 2.
the kinetic energy will increase by a factor of 4 because velocity is squared in the equation for KE
79
relationship between temperature, average KE, and average velocity
as temperature increases, so does KE and velocity
80
Kinetic eneregy is also known as what kind of energy
thermal energy
81
what does elastic mean when discussing collision of particles
when two particles collide, energy is exchanged, but there is no overall loss or gain of energy
82
how is rate of effusion related to mass, speed?
rate of effusion is inversely related to mass, but directly related to speed
83
describe the relationship between KE and pressure
pressure is proportional to average KE
84
formula for kinetic energy
KE(ave) = 1/2m * v^2(ave)
