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KLowe Chemistry And Physics Larmon > Gas Laws > Flashcards

Gas Laws Flashcards

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1
Q

Empirical gas laws describe…

A

The 4 quantities that describe the state of a gas:

  • Pressure
  • Temperature
  • Volume
  • Number of moles
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2
Q

STP =

A

Standard temperature and pressure

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3
Q

Standard temperature =

A

273 K (0 degrees Celsius)

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4
Q

Standard pressure =

A

1 atm = 760 mm Hg

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5
Q

Standard molar volume—At STP, one mole of (an ideal) gas has a volume of ___

A

22.414 L (new books may list 22.7 L)

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6
Q

3 empirical gas laws:

A
  • Boyle’s Law
  • Charles’s Law
  • Avogadro’s Law
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7
Q

Boyle’s Law =

A

P1V1 = P2V2

Volume is inversely related to pressure (at constant n and T)

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8
Q

Charles’s Law =

A

V1/T1 = V2/T2

Volume is directly proportional to the absolute temperature (constant n and P)

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9
Q

Avogadro’s Law =

A

The volume of a gas is directly proportional to the number of gas molecules (constant T and P)

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10
Q

Boyle’s Law = ___ relationship

A

Volume-Pressure relationship

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11
Q

Boyle’s law forms the basis of the relationship between the three important parameters of a gas…

A
  • Volume
  • Pressure
  • Temperature
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12
Q

Boyle’s Law—the volume of a fixed sample of gas is inversely related to ___, as long as ___ is constant

A

Pressure, temperature

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13
Q

Boyle’s law—as pressure increases, volume ___

A

Decreases

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14
Q

Boyle’s law—as pressure decreases, volume ___

A

Increases

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15
Q

Boyle’s law is the basis of ___

A

Breathing

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16
Q

Boyle’s law formula

A

P1V1 = P2V2

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17
Q

Charles’ work was the basis of ___

A

The ideal gas law

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18
Q

Charles’ Law is also known as the ___

A

Law of volumes—describes how gases expand in volume when heated

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19
Q

Charles’ Law states that the volume of an ideal gas is proportional to ___

A

Its absolute temperature under constant pressure

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20
Q

Charles’ Law changes ___ of gas molecules

A

Kinetic energy

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21
Q

Charles’ Law—if absolute temperature of a gas doubles, ___ doubles

A

Volume

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22
Q

Charles’ Law—if temp is halved, volume ___

A

Halved

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23
Q

Charles’ Law formula

A

V1/T1 = V2/V2

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24
Q

Kelvin scale for Charles’ Law

A

K = Degrees Celsius + 273

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25
Q

Charles’ Law—temperature corresponding to V = 0

A

Must be the coldest possible temperature—this temperature is called absolute zero

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26
Q

Charles’ Law example—cuff volume ___ in an ETT placed in a patient

A

Increased cuff volume with increased patient body temperature

Can result in increased mucosal pressure and integrity

Concern in pediatric patients; could cause subglottic stenosis

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27
Q

Avogadro—the ___ relationship

A

Volume-mole relationship

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28
Q

Avogadro’s number =

A

6.022 x 10^23

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29
Q

Avogadro’s Law—at equal temperatures and pressures, equal volumes of gas contain ___ numbers of particles; the volume of gas is directly proportional to ___, as long as pressure and temperature are held constant

A

Equal; number of gas molecules

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30
Q

Avogadro’s Law formula

A

V1/n1 = V2/n2

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31
Q

At STP, one mole of (an ideal) gas has a volume of ___

A

22.414 L (22.7 L)

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32
Q

Gay-Lussacs Law formula

A

P1/T1 = P2/T2

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33
Q

Gay-Lussacs Law—pressure is directly proportional to ___ if volume is constant

A

Temperature

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34
Q

Gay-Lussacs Law—as temperature goes up, pressure ___

A

Goes up (if volume is constant)

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35
Q

Gay-Lussacs example—N2O cylinder

A

As gas is released, liquid in tank vaporizes; heat is lost; temperature in cylinder falls and pressure drops (temperature affects pressure on constant volume cylinder)

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36
Q

Ideal gas law

A

Combines the elements of the empirical gas laws to formulate a state function to completely describe the state of a gas under a given set of conditions

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37
Q

Formula for ideal gas law

A

PV = nRT

P = pressure
V = volume
N = number of moles
T = absolute temperature
R = constant
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38
Q

Ideal gas law—volume is inversely proportional to ___

A

Pressure

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39
Q

Ideal gas law—volume is directly proportional to ___

A

Absolute temperature, moles

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40
Q

R =

A

Universal gas constant

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41
Q

Most common R = (#)

A

0.08205

42
Q

R describes the relationship between ___ and ___

A

Temperature and kinetic energy

43
Q

The value of R in SI units =

A

8.314 J/mol/K

44
Q

Gas density depends strongly on ___ and ___

A

Temperature and pressure

45
Q

What is partial pressure?

A

The pressure exerted by an individual gas in a mixture

46
Q

Dalton’s law of partial pressures

A

The total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases

47
Q

Relative humidity measures…

A

The saturation of water in air (mass of water in the air/mass of water that WILL FIT in the air)

48
Q

Do ideal gases exist?

A

No

49
Q

Kinetic molecular theory of gases

A

Based on the four basic tenets which exactly describe an ideal gas

Assumes that molecules are very small relative to the distance between molecules; the molecules are in constant, random motion and frequently collide with each other and with the walls of any container

50
Q

Kinetic molecular theory of gases—1) Gases consist of…

A

Small particles whose volume is negligible compared to the volume of the gas

51
Q

Kinetic molecular theory of gases—2) Gas molecules are in ___ motion

A

Constant, random

52
Q

Kinetic molecular theory of gases—3) The molecules in the sample show a range of kinetic energies, but the average KE depends only on ___

A

Temperature

53
Q

Kinetic molecular theory of gases—4) There are no ___ between gas particles, so all collisions are elastic

A

Attractive or repulsive forces between the gas particles

54
Q

What is the density of a gas?

A

D = M/V

55
Q

Pressure of a gas measures ___

A

Linear momentum of the molecules

56
Q

Pressure =

A

Force/area

57
Q

Temperature of a gas

A

Measure of the mean kinetic energy of the gas

58
Q

The higher the temperature, the ___ motion

A

Greater the motion

59
Q

Internal energy

A

Sum of kinetic and potential energy

60
Q

Temperature is directly proportional to ___

A

Average KE

61
Q

The average KE is the same for gases at the same ___

A

Temperature

62
Q

Different gases have the same average KE if…

A

Their temperatures are the same

63
Q

Diffusion

A

Movement of a substance from an area of higher concentration to an area of lower concentration

64
Q

Effusion

A

Movement of a gas through a small opening

65
Q

Graham’s Law of Effusion—The rate of effusion is inversely proportional to ___

A

The rate of effusion is inversely proportional to the square root of the molecular mass

66
Q

The rate of effusion depends on the ___

A

Speed of the molecules

67
Q

Fick’s Law—the rate of diffusion of a gas across a permeable membrane is determined by what 4 things?

A
  • Chemical nature of the membrane itself
  • Surface area of the membrane
  • Partial pressure gradient of gas across the membrane
  • Thickness of the membrane
68
Q

Diffusion rate of a gas is directly proportional to (3)…

A
  • Partial pressure gradient
  • Membrane area
  • Solubility of gas in membrane
69
Q

Diffusion rate is inversely proportional to (2)…

A
  • Membrane thickness

- The square root of the molecular weight

70
Q

Diffusion-limited gas exchange describes the scenario in which the rate at which gas is transported away from functioning alveoli and into tissues is principally limited by ___

A

The diffusion rate of the gas across the alveolar membrane

71
Q

Perfusion-limited gas exchange describes the scenario in which the rate at which gas is transported away from functioning alveoli and into tissues is principally limited by ___

A

The rate of blood flow through the pulmonary capillaries and thus across the alveolar membrane

72
Q

Diffusion- and perfusion-limited gas exchange are distinguished by the extent that an alveolar gas’ ___ as blood ___

A

Partial pressure will equilibrate across the alveolar membrane as blood flows through the pulmonary capillaries

73
Q

Nitrous oxide perfusion-limited gas exchange

A

The idea that the partial pressure of nitrous oxide equilibrates rapidly, eliminating the partial pressure gradient across the alveolar membrane long before blood reaches the end of the capillaries. The principle factor limiting blood transport of N2O away from the lungs is the rate of blood flow through the pulmonary capillaries (perfusion-limitation)

74
Q

The rate of diffusion of a substance across unit area (such as a surface or membrane) is proportional to the ___

A

Concentration gradient

75
Q

Fick’s law of diffusion for gases explains (4):

A
  • The concentration effect
  • The second gas effect
  • Diffusion hypoxia
  • Why N2O leads to increase in volume or increase in pressure in gas spaces in the body
76
Q

CO2 is ___ than O2

A

Larger

77
Q

CO2 diffuses ___ faster than O2

A

20x’s — because it is 20x’s more soluble

78
Q

Equilibration of an inhalational agent occurs in the body when the partial pressure of the gas is ___

A

The same everywhere

79
Q

The process by which the fetus receives O2 and drugs is ___

A

Simple diffusion across a membrane

80
Q

Diffusion of a gas from alveoli to blood (or back out) requires a difference in ___

A

Partial pressures

81
Q

Henry’s Law—the amount of a non-reacting gas which dissolves in liquid is directly proportional to the ___, provided the temperature remains constant

A

Partial pressure of the gas

82
Q

Dissolved O2 in blood =

A

0.003ml/100ml/mmHg partial pressure of O2

Calculate—multiply pp of O2 by 0.003

83
Q

Dissolved CO2 in blood =

A

0.067ml/100ml blood/mmHg partial pressure of CO2

Calculate—multiple pp of CO2 by 0.067

84
Q

The amount of gas dissolved is inversely proportional to ___

A

Temperature

85
Q

The colder the liquid, the ___ gas that will dissolve in the liquid

A

More

86
Q

Ostwald’s Solubility Coefficient

A

The quantity of solvent needed to dissolve a quantity of gas at a given temperature and pressure

87
Q

Ostwald’s solubility coefficient—the higher the coefficient, the ___ gas dissolves in the liquid

A

More readily (i.e.: blood/gas)

The two phases must be specified

88
Q

Higher partition coefficient = ___ lipophilicity = ___ potency = ___ solubility

A

Higher lipophilicity, higher potency, higher solubility

89
Q

High solubility = ___ anesthetic needs to be dissolved = ___ onset

A

More anesthetic, slower onset

90
Q

MAC ___ as blood gas partition coefficient increases

A

Decreases

91
Q

Meyer Overton rule

A

Agents with increased oil solubility have greater potency (d/t a cell’s lipid membranes)

92
Q

Ideal gases obey gas laws at all ___

A

Temps and pressures

93
Q

Do ideal gases exist?

A

No

94
Q

Real gases deviate at ___

A

High pressure and/or low temps

95
Q

What equation deals with the deviations in real gases?

A

Vander Waals

96
Q

Vander Waals relationship assumes that gas molecules have ___ volumes and gas molecules ___ one another

A

Finite volumes, attract one another

97
Q

Joule-Thompson Effect—thermodynamic process that occurs when a fluid ___ from high pressure to low pressure at constant enthalpy. Under the right conditions, this can cause ___ of the fluid

A

Expands, cooling

98
Q

Examples of the Joule-Thompson Effect—as a cylinder of compressed gas empties, the cylinder ___

A

Cools

Other examples: how a cryoprobe works, N2O tanks

99
Q

Adiabatic compression

A

Compression in which no heat is added to or subtracted from the air and the internal energy of the air is increased by an amount equivalent to the external work done on the air

AKA — compression that increases the internal energy of the air by external work done on the air

100
Q

Adiabatic compression—the increase in temperature of the air during adiabatic compression tends to increase the ___ on account of the ___ in volume alone

A

Pressure, d/t decrease in volume

101
Q

Reaction of CO2 in soda lime

A

CO2 + H2O —> H2CO3

H2CO3 + 2NaOH —> Na2CO3 + 2H2O + heat

Na2CO3 + Ca(OH)2 —> CaCO3 + NaOH

KLowe Chemistry And Physics Larmon (11 decks)

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