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P&P Fall 2019 > Gas Laws > Flashcards

Gas Laws Flashcards

1
Q

Lipophilic drugs are ionized or nonionized?

A

Nonionized

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2
Q

Hydrophilic drugs are ionized or nonionized?

A

Ionized

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3
Q

Gases: molecules are _______, ____ amount of disorder

A

molecules not in contact

high disorder

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4
Q

Lighter gases diffuse more or less rapidly than heavy ones?

A

Diffuse more rapidly

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5
Q

Diffusion is the process of _____

A

in which gases move from an area of high concentration to low concentration

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6
Q

______ occurs when the partial pressures of the gas are the same throughout the body

A

equilibration

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7
Q

What is required in order for diffusion of a gas from the alveoli to the blood to occur?

A

a partial pressure difference

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8
Q

Ficks Law of diffusion

A

Diffusion Rate =

P1-P2)(Area)(Solubility) / (membrane thickness)(Square root of MW

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9
Q

Clinical applications of Ficks law

A
  • concentration effect
  • second gas effect
  • diffusion hypoxia
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10
Q

Concentration effect

A

“overpressurizing” - initially a higher concentration of volatile than necessary (loading dose) delivered to speed initial uptake

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11
Q

Second Gas Effect

A

simultaneous administration of slow agent (volatile) and faster agent (N2O) speeds onset of slower volatile

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12
Q

Diffusion Hypoxia

A

during emergence when high concentrations of rapid anesthetic (N2O) are given, agent exits quickly thru lungs and replaced by less soluble nitrogen in air – pt may desat d/t transient dilution of O2 & CO2

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13
Q

Grahams Law

A

rate of diffusion of a gas is inversely proportional to the square root of the MW –> the heavier the molecule, the slower the diffusion
R=1/sq root MW

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14
Q

pressure =

A

force per unit area

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15
Q

How do gases create pressure?

A

force exerted by molecules when they collide w/in certain area of closed container

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16
Q

1mmHg = _______ cmH20

A

1.36 cm H20

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17
Q

1 atm = _____ mmHg

A

760 mmHg

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18
Q

1 atm = _______ psi

A

14.7psi

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19
Q

1 psi = ______ mmHg

A

54 mmHg

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20
Q

What is atmospheric pressure at sea level?

A

760mmHg or 1034 cm H2O

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21
Q

% concentration =

A

Grams per 100 mL

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22
Q

1:1000 =

A

1 gram in 1000mL

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23
Q

1:1000 = how many mcg/mL?

A

1mg/mL or 1,000mcg/mL

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24
Q

1kg = ______N

A

10 Newtons

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25
Q

10 Newton = _____ lbs

A

2.25lbs

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26
Q

Cricoid pressure is how much?

A

44 N or 10 lbs

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27
Q

Critical Temperature

A

gases liquefy if sufficient pressure is applied & temperature is below a critical temperature
–> a gas cannot be liquefied if it is not below temp, no matter the pressure applied

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28
Q

Critical Temperature of N20

A
  1. 5C

- -> therefore can be compressed & stored as liquid at room temp

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29
Q

Critical Temperature of O2

A

119C

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30
Q

Capacity of full E cylinder

A

625-700L

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31
Q

Pressure of full E cylinder

A

1800-2200 psi

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32
Q

Medical gas system - oxygen - stored via pipeline with what pressure?

A

2000 +/- 5 psi

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33
Q

How to calculate time to empty full Ecylinder?

A

Volume/Flow=Time

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34
Q

If the flow of O2 from an Ecylinder is 5L/min, how long will it take to empty a full cylinder?

A

625/5= 125 minutes

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35
Q

Full cylinder of N20 contains ______L at ____ psi

A

1590L

725-750 psi

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36
Q

How is nitrous oxide stored?

A

Liquefied

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37
Q

Joule-Thompson Effect

A

As gas escapes from N20 cylinder, liquid N20 vaporizes, heat is lost, temp of cylinder falls

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38
Q

N20: as the cylinder temp _____, the pressure of the gas in the cylinder ______

A

decreases, decreases

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39
Q

Latent heat of melting

A

converts solid to liquid

40
Q

latent heat of vaporization

A

converts liquid to a gas

41
Q

latent heat of condensation

A

converts gas to liquid

42
Q

latent heat of crystallization

A

converts liquid to a solid

43
Q

Occurs at constant temperature from vapor molecules bombarding the walls of the container

A

Saturated Vapor Pressure

44
Q

volatile anesthetic agents are liquids that have ____

A

an inherent tendency to change to a vapor at standard temperature and pressure

45
Q

______ the volatility of an agent, ______ the tendency to enter the vapor phase

A

Higher; stronger

46
Q

Increased volatility = _____

A

higher vapor pressure

47
Q

Desflurane Vapor Pressure

48
Q

Isoflurane Vapor Pressure

49
Q

Sevoflurane Vapor Pressure

50
Q

Enflurane Vapor Pressure

51
Q

Halothane Vapor Pressure

52
Q

Vapor pressure, independent of atmospheric pressure, is a function of _____

A

temperature

53
Q

Heat will ______ vapor pressure

54
Q

Cooling wil ______ vapor pressure

55
Q

Absolute humidity

A

mass of water vapor in a given volume of air

56
Q

Relative humidity

A

(actual vapor pressure/saturated vapor pressure) X 100

57
Q

Partial pressure of saturated water vapor at 37C

58
Q

Bourdon Gauges measures ______

A

The pressure relative to atmospheric pressure (measures the cylinder pressure)

59
Q

When bourdon gauge = 0

A

pressure in cylinder is same as atmospheric

60
Q

Law of LaPlace

A

As radius increases, tension (force) of wall of structure increases

61
Q

The ______ the radius in a chamber or vessel, the ______ the tension in the walls of the chambers or vessels

A

greater; greater

62
Q

Clinical application of Law of LaPlace

A
  • Aortic aneurysm is more likely to rupture d/t larger radius
  • Heart: greater filling in ventricle, greater tension in ventricle wall
  • Veins > capillary tension
63
Q

Law of LaPlace Equation

A

T = DeltaP x R

Wall tension = pressure of liquid w/in cylinder x radius

64
Q

Law of LaPlace Equation for Spheres

65
Q

Clinical application for Law of LaPlace - Spheres

66
Q

Normal Alveoli - pressure and tension

A

P1=P2 because T1 < T2

67
Q

ARDs or surfactant deficient alveoli - pressure and tension

A

P1 > P2 because T1=T2

68
Q

Poiseulle’s Law

A

describes laminar (streamlined) flow

69
Q

Poiseulle’s Law Equation

A

F (volume flow rate) is directly proportional to the 4th power of the radius

70
Q

Poiseulle’s Law is affected by

A 
Length of tube (inversely)
Viscosity (inversely)
change in pressure (directly)
radius (directly)
...these all effect the volume flow rate
71
Q

Poiseulles Law - clinical application related to pressure

A

raising the IV pole – increases hydrostatic pressure and increases flow

72
Q

Poiseulles Law - clinical application related to viscosity

A

polycythemic patients have high blood viscosity, flow through blood vessels is reduced

73
Q

Reynold’s number

A

predicts when flow thru cylindrical tube changes from laminar to turbulent

74
Q

Reynold’s number > 1500-2000

A

flow changes from laminar to turbulent

75
Q

When flow is turbulent, ______ determines flow

76
Q

When flow is laminar, ______ determines flow

77
Q

Bernoulli’s Principle

A

Venturi Effect - when fluid flows thru a constricted region of tube, the velocity of flow increases and the lateral pressures decreases

78
Q

Henry’s Law determines what

A

permits calculation of dissolved O2 and dissolved CO2; the amount of a gas in a liquid is proportional to the partial pressure of the gas in the gas phase

79
Q

How much does dissolved O2 increase in the blood when PaO2 increases from 100mmHg to 500 mmHg

A

100 mmHg x 0.003 = 0.3 mL O2/100mL blood
500 mmHg x 0.003 = 1.5 mL O2/100mL blood
SO
Dissolved O2 increased 1.2mL O2/100mL blood

80
Q

Henry’s Law - if given inspired O2, estimate PaO2 how?

A

multiply inspired concentration by 5

81
Q

Henry’s Law - if given inspired O2, estimate PaO2 how?

i.e. how much O2 is dissolved if FiO2 is 40%?

82
Q

Amount of Co2 that dissolved in blood

A

0.06 mL/100mL blood/mmHg

83
Q

Amount of O2 that dissolved in blood

A

0.03 mL/100mL blood/mmHg

84
Q

Boyles Law

85
Q

Boyles Law - Clinical application

A

Ambu Bag squeezed - raises pressure and decreases volume

86
Q

Charles Law

A

V1/T1=V2/T2

87
Q

Charles Law Clinical application

A

helium balloon outside on cold day will deflate, bring it inside to warmth & it will inflate again

88
Q

Charles Law - how to calculate:

at 15dC a gas occupies a volume of 273 mL. At 30dC, what volume will that gas occupy?

A

273mL/15dC=XmL/30dC

546mL

89
Q

Gay Lussac’s Gas Law

A

P1/T1=P2/T2

90
Q

Joule Thompson Effect

A

When the gas escapes the cylinder, liquid continues to vaporize into the space above, exerts same pressure onto walls until liquid disappears. Vaporization requires heat and the liquid cools

91
Q

ideal gas law

A

PV=nRT

avogadros

92
Q

Daltons Law

A

total pressure in mix of gases is equal to the sum of pressures in individual gases (each gas exerts a partial pressure)

93
Q

how to calculate partial pressure of gas

A

Percent concentration*Atmospheric pressure

94
Q

How to estimate PAO2 (alveolar)

A

Percent inspired O2*6

95
Q

V/Q mismatch

A

If PA02-PaO2 = not FiO2

P&P Fall 2019 (17 decks)

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