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Chemistry I > Chapter 6: Gases > Flashcards

Chapter 6: Gases Flashcards

1
Q

volume of a gas equal the volume of its BLANK

A

container

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2
Q

gases have neither fixed BLANK nor BLANK

A

shape or volume

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3
Q

all gases form BLANK mixtures

A

homogeneous

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4
Q

describe level of interaction of gas molecules

A

gas molecules have little interaction, they are relatively far apart from each other

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5
Q

formula for gas pressure

A

force dvided by area

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6
Q

in a liquid, gases occupy how much of the space

A

70%

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7
Q

what does STP stand for

A

Standard Atmospheric Pressure

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8
Q

1 atm equals how many mmHg/Torr

A

760 mmHg and 760 Torr

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9
Q

how are volume and pressue related in gas laws

A

inversely related

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10
Q

what is Boyle’s Law

A

gas volume is inversely proportional to pressure

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11
Q

Boyle’s law formula

A

V1P1=V2P2

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12
Q

what is Charles’s Law

A

gas volume is directly proportional to Kelvin temperature

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13
Q

Charles’s Law formula

A

V1/T1=V2/T2

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14
Q

Avogadro’s Law

A

voume of gas is proportional to molar amount

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15
Q

Avogadro’s Law formula

A

V1/n1=V2/n2

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16
Q

what is the gas constant in IGL

A

r = .08206 Latm/molk

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17
Q

IGL standard temperature for gas

A

t= 0° C

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18
Q

standard pressure for gas IGL

A

P = 1 atm

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19
Q

IGL for volume

A

Liters

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20
Q

IGL unit for pressure

A

atm

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21
Q

IGL unit for temperature

A

Kelvin

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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

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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

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24
Q

Dalton’s Law formula

A

P(total) = P(A) + P(B) + P(C)…

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25
Q

IGL equation

A

PV = nRT

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26
Q

mole fraction equation

A

X(A) = P(A)/P(total)

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27
Q

what does KMT stand for

A

kinetic molecular theory

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28
Q

what is KMT

A

model that explains behavior of gases

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29
Q

In KMT, gas consists of particles in what kind of motion

A

constant, random motion

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30
Q

In KMT, the size of gas particles is BLANK compared to the size of container

A

the size is negligible

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31
Q

In KMT, the strength of intermolecular forces is BLANK

A

negligible

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32
Q

In KMT, the average KE of gas particles is directly proportional to what?

A

Kelving temperature

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33
Q

In KMT, all collisions of the gas particles are BLANK. What does this mean?

A

Alll collisions are elastic, meaning there is no loss of KE

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34
Q

A real gas will have properties most like an idea gas at what temperature and pressure?

A

high temperature and low pressure

35
Q

real gases differ from idea gases in that…

A

real gases have volume and particles that interact and collide

36
Q

speed at which a molecules is traveling depends on what two things?

A

speed depends on mass of the molecule and temperature

37
Q

the lighter a gas particle, the BLANK the speed

A

faster the gase’s speed

38
Q

formula for rms speed

A

u = √3RT / √M

39
Q

what is effusion

A

escape of gas through a tiny orifice into an evacuated chamber

40
Q

what is Graham’s Law of effusion

A

rate of effusion is inversely proportional to the square root of the molar mass

41
Q

what is diffusion

A

the mixing of two gases, from higher concentration to lower concentration

42
Q

what is effusion rate?

A

the faster the particles move, the more likely they are to pass through the effusion orifice

43
Q

deviations from idea gas behavior are largest when pressure is BLANK and temperature is BLANK

A

when pressure is high and temperature is low

44
Q

when pressure is high, size becomes BLANK

A

significant

45
Q

when temperature is low, attractive forces become BLANK

A

significant

46
Q

what does “n” equal?

A

amount of gas in moles

47
Q

in a J-tube, the height of Hg is proportional to what?

A

the pressure of the gas

48
Q

define molar volume

A

volume occupied by 1 mole of a substance at T=0° C / 273.15 K and P=1atm

49
Q

define pressure

A

amount of force per unit area

50
Q

relationship between concentration and pressure

A

direct relationship: lower concentration=lower pressure

51
Q

what is pressure measured with

52
Q

what is atmospheric pressure

A

average pressure at sea level

53
Q

what do simple gas laws describe

A

relationship between P, V, T, and n

54
Q

what does extrapolate mean

55
Q

what did Charles quantify?

A

relationship between volume and temperature

56
Q

what happens to speed of particles when temperature increases?

A

particles move faster

57
Q

the molar volume of a gas of 22.414 L only applies at what?

A

standard temperature and pressure

58
Q

density of a gas equals

A

molar mass divided by molar volume

59
Q

formula for molar gas

A

molar mass = mass/moles

60
Q

describe the interaction of molecules in an ideal gas

A

molecules in an IG do not interact

61
Q

general gas law formula

A

P1V1/T1 = P2V2/T2

62
Q

one mole of an ideal gas at STP has a volume of what?

63
Q

according to KMT, when gas density is very low…

A

particles are far apart

64
Q

the IGL are most valid when…

A

when particle density is very low

65
Q

when particle density is very low…

A

the distance between particles is greater than the particle size

66
Q

describe kinetic energy at high temperatures

A

kinetic energy or particles is much greater than the strength of intermolecular forces

67
Q

what is assumed of gas particles when kinetic energy is very high

A

it is assumed that gas particles don’t interact, other than random collisions

68
Q

describe the distance of gas particles at low pressures

A

gas particles are far away from each other

69
Q

when gas particles are far away from each other, what is assumed?

A

the size of gas particles is negligible

70
Q

observations lead to what?

71
Q

what does kinetic molecule theory do for gas laws

A

KMT provides reasons behind the laws

72
Q

what is a gas

A

collection of particles in constant motion

73
Q

when particle size is negligibly small, what can be said of volume?

A

the particles don’t occupy volume

74
Q

average kinetic energy depends ONLY on what?

A

temperature of gas

75
Q

Can the speed of a GIVEN molecule in a gas double at constant temperature? Explain your answer.

A

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
Q

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.

A

average kinetic energy with remain constant due to constant temperature

77
Q

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.

A

Av. KE will increase because temperature increased

78
Q

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.

A

the kinetic energy will increase by a factor of 4 because velocity is squared in the equation for KE

79
Q

relationship between temperature, average KE, and average velocity

A

as temperature increases, so does KE and velocity

80
Q

Kinetic eneregy is also known as what kind of energy

A

thermal energy

81
Q

what does elastic mean when discussing collision of particles

A

when two particles collide, energy is exchanged, but there is no overall loss or gain of energy

82
Q

how is rate of effusion related to mass, speed?

A

rate of effusion is inversely related to mass, but directly related to speed

83
Q

describe the relationship between KE and pressure

A

pressure is proportional to average KE

84
Q

formula for kinetic energy

A

KE(ave) = 1/2m * v^2(ave)

Chemistry I (16 decks)

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