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GNUS561- Chem & Physics > Gas Law's-Quiz 4 > Flashcards

Gas Law's-Quiz 4 Flashcards

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1
Q

What is the partial pressure of DES?

A

669

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2
Q

What does Vander Waals Equation correct for?

A

Intermolecular attractions between gases and for the finite volume of the gas molecule.

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3
Q

T/F: even though CO2 is larger than O2, CO2 diffuses 20x faster across the alveolar and capillary membranes.

A

True. Because it is 20x more soluble.

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4
Q

Step 3. Na2CO3 + Ca(OH)2 (calcium hydroxide) ->

A

CaCO3 (calcium carbonate) + NaOH (sodium hydroxide)

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5
Q

Gaseous water molecules create a “vapor pressure. “ At higher temperature, more water vaporizes and exerts a greater vapor pressure. What is this relationship?

A

Maximum solubility of water in the air is directly related to vapor pressure of water.

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6
Q

Fick’s Law essentially states that the rate of diffusion of a gas across a permeable membrane is determined by what?

A
  • chemical nature of the membrane itself
  • surface area of the membrane
  • partial pressure gradient of gas across the membrane
  • thickness of the membrane
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7
Q

What does Henry’s Law state?

A

The amount of a non reacting gas which dissolved in a liquid is directly proportional to the partial pressure of the gas, provided the temperature remains constant.

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8
Q

The process by which the fetus receives O2 and drugs across a membrane is by what?

A

Simple diffusion

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9
Q

The kinetic theory of gases assumes that molecules are ______ relative to the distance between molecules.

A

Small. Molecules are in constant, random motion and frequently collide with each other and with the walls of any container.

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10
Q

What is Standard Molar Volume?

A

-At STP, one mole of (an ideal) gas has a volume of 22.414L

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11
Q

HLH (High Low High) means what in Don terms?

A

If a high vapor pressure agent is put in a vaporizer designed for a lower pressure agent the concentration of the agent delivered will be higher. And vice versa for LHL.

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12
Q

What is the volume - mole relationship ?

A

Volume% = mole%
At STP one mole of an ( ideal gas has a volume of 22.414L)
- 0.5 mole has volume 11L
-3 mole of a gas has 66L

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13
Q

Kinetic Molecular Theory of Gases: What is density?

A

The sum of the mass of the molecules divided by the volume which the gas occupies.

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14
Q

What is the partial pressure of ISO?

A

240

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15
Q

Dissolved O2 in the blood is

A

0.003ml/100ml blood/mmHg partial pressure of O2

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16
Q

The mole fraction is a way of expressing the relative proportion of one particular gas within a mixture, how do we calculate this?

A

Dividing the number of moles of a particular gas by the total number of moles in a mixture

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17
Q

Kinetic Molecular Theory of Gases: What is temperature?

A

A measure of the mean kinetic energy of the gas. Molecules are in constant random motion, there is energy associated with the motion. Higher the temperature, the greater the motion.

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18
Q

What is the partial pressure of N20 and O2 if they are delivered to the patient in a 70/30 mixture?

A

N20= ( 0.7 x 760 mmgHg = 532 mmHg)

O2 ( 0.3 x 760) = 228

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19
Q

Kinetic Molecular Theory of Gases: What is pressure?

A

A measure of the linear momentum of molecules. As gas molecules collide with the walls of a container, the molecules impart momentum to the walls, producing a force that can be measured. The force divided by the area is pressure.

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20
Q

Describe Charle’s Law

A

V1/T1 = V2/T2

  • Volume and temperature are directly proportional
  • At a constant pressure and n
  • Ex: ETT cuff, LMA, increase in Temperature expands the VOLUME
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21
Q

Diffusion rate of a gas is directly proportional to

A
  • Partial pressure gradient
  • Membrane Area
  • Solubility of gas in membrane
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22
Q

How do you calculate the O2 dissolved in the blood?

A

Multiply 0.003 by the partial pressure of O2 on the blood gas

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23
Q

Diffusion rate is inversely proportional to

A
  • membrane thickness

- the sq root of the molecular weight

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24
Q

If the air is gradually cooled while maintaining the moisture content constant, the relative humidity will rise until it reaches 100%. This temperature at which the moisture content in the air will saturate the air is called what?

A

Dew point

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25
Q

IF the pressure on the gas isn’t too high and the temperature isn’t too low, what do real gases do?

A

Approximate ideal behavior

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26
Q

What is the value of R, the universal gas constant?

A

= 0.0821 L atm/ k / mole ( apex)

= 0.082057 Don

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27
Q

What are clinical examples of Boyles law ?

A
  • INHALE, intrathoracic pressure goes down ( pressure) tidal volume of lung goes UP
  • Exhale intrathoracic pressure goes UP and atmospheric pressure ( lung volume) goes DOWN
  • ** His review at the end of class
  • Squeeze of Ambu bag increases pressure, decreases volume
  • Plethysmography ( measurement of FRC )
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28
Q

RH and temperature

- If there is a fixed amount of water in the air, and the temperature decreases how does the relative humidity change?

A

The relative humidity increases.

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29
Q

Fick’s Law of Diffusion and Nitrous Oxide

A

A rapid diffusion rate across the alveolar membrane and is not bound by any proteins within blood. The gas partial pressure of N2O within blood rises rapidly following the transport of only minimal amounts of the gas.

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30
Q

What is Dalton’s Law of Partial Pressures>?

A

The pressure exerted by an individual gas in a mixture is known as its partial pressure.

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31
Q

The average kinetic energy depends only on what?

A

Temperature.

Temperature and Pressure are proportionally related.

32
Q

Describe Gay- Lussac’s Law

A

P1/T1=P2T2

  • Pressure and temperature are directly proportional
  • At a constant volume and n
  • Ex: N2O cylinder, as gas is released the liquid in the tank vaporizes = Heat is lost , decrease in temperature, the PRESSURE decreases
33
Q

What is the partial pressure of SEVO?

A

157 or 160

34
Q

What is 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. The increase in temperature of the air during compression tends to increase the pressure on account of the decrease in volume alone.

35
Q

What is another equation to express RH?

A

RH= PH20/ VP of water

Divide the amount of water in air by the solubility of the water in the air

36
Q

What values do we need to know if Standard pressures 1atm

A

= 760 mmHg = 760 torr = 1 bar = 100kPa = 1033 cm H20 = 14.7 lb/inch ^2 = WAS 1 standard mole volume 22.4 NOW 22.71 L

37
Q

What is the Diffusion-Limited Gas Exchange?

A

The rate at which gas is transported away from functioning alveoli and into tissues is principally limited by the diffusion rate of the gas across the alveolar membrane.

38
Q

Warmer air holds more water, if the air cools what happens to the concentration of water in the air?

A

It increases

39
Q

Fick’s Law of Diffusion for gases explains:

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.
40
Q

The Law of Volume

T/F: Volume of an ideal gas is inversely proportional to its absolute temperature under a constant pressure?

A

False- Directly proportional

  • *This is explained by molecular motion
  • Increase/ Decrease temperature from energy added or taken away changes kinectic energy of gas molecules = Volume changes
41
Q

T/F: the amount of gas dissolved is inversely proportional to temperature?

A

True. The colder the blood more gas will dissolve and can prolong emergence. Vice Vera’s is also true. Normothermia is important!

42
Q

What is Ostwald’s Solubility Coefficient?

A

The quantity of a solvent needed to dissolve a quantity of gas at a given temperature and pressure. The higher the coefficient the more readily the gas dissolved in the liquid. (i.e. blood:gas coefficient)

43
Q

T/F: effusion and diffusion are substantially the same process

A

True

44
Q

What are Standard Conditions?

A 
STP= Standard temperature and pressure 
T= 273.15 K or O degres celsius
P= 1.00 atm = 760 torr ( = 760mmHg/ apex)
45
Q

What is the Universal Gas Law?

A 
Combines the elements or empirical gas laws to formulate a state of function to completely describe the sate of a gas under a given set of conditions 
PV = nRT
P= Pressure
V= Volume
n= Number of moles
T= Absolute temperature
R is a constant
***Conceptually think of P= T/V ( apex)
46
Q

What is the partial pressure of O2 in the mountains if Patm is 550mmHg?

A

O2 ( 0.21 x 550) = 116

47
Q

What happens if the absolute temperature of a gas doubles?

A

The volume will doubles

48
Q

What is the partial pressure of CO2 if the end-tidal gas is 5%?

A

CO2 ( 0.05 x 760) = 38 mmHg

49
Q

Unlike liquids or solids, what does Gas density strongly depend on?

A

Temperature and Pressure

50
Q

Describe Boyle’s Law

A

P1V1=P2V2

-Pressure and volume are INVERSELY related -At a constant temperature and n

51
Q

Carbon Dioxide Absorber involves a reaction of CO2 in what?

A

Soda Lime

52
Q

T/F: Higher Solubility = less anesthetic needs to be dissolved and slower onset.

A

False. MORE anesthetic needs to be dissolved and slower onset

53
Q

The sum of the kinetic energy and potential energy is that what?

A

Internal Energy

54
Q

Meyer Overton states what?

A

Agents with increased oil solubility have greater potency. This is due to a cells lipid membranes. Smaller amount of gas needed to obtain MAC when the oil solubility is higher.

55
Q

What does Daltons law state?

A

The total pressure mixture of gases is equal to the sum of the partial pressures of the gas component
PTotal = p1 + P2 + P3

56
Q

What 4 quantities are in the Empirical Gas Laws?

A

1-Pressure
2-Volume
3- Volume
4-Number of moles

57
Q

Key points to Ostwald’s Solubility: Higher partition coefficient=

A

Higher lipophilicity = higher potency = higher Solubility

58
Q

Step 1. CO2 + H2O ->

A

H2CO3 (carbonic acid)

59
Q

What is Avogadro’s Number?

A
  1. 023 x 10 ^23 atoms
    - Hypothesis is that, at equal temperatures and pressures, equal volumes of a gas contain equal number of particles

**APEX: A mole of a gas is equal to the molecular weight of that gas in grams

60
Q

MAC decreases as the blood gas partition coefficient does what?

A

Increases. (Generally speaking)

61
Q

What is diffusion?

A

The movement of a substance from an area of higher concentration to an area of lower concentration.

62
Q

What is Avogadro’s Law?

A

The volume of a has is DIRECTLY proportional to the number of gas molecules ( at constant T and P)
-More gas molecules = bigger volume

63
Q

How do you calculate the amount of CO2 dissolved in the blood?

A

Multiply 0.067 by the partial pressure of CO2 on the blood gas

64
Q

Graham’s Law of Effusion is inversely proportional to the square root of what?

A

Molecular Mass. -> smaller molecules will effuse quicker

65
Q

What is effusion?

A

The movement of a gas through a small opening.

66
Q

T/F: Ideal gases do exist?

A

False

- Ideal gases do not exist

67
Q

Step 2. H2CO3 + 2 NaOH (Sodium Hydroxide) ->

A

Na2CO3 (Sodium Carbonate) + 2H2O + Heat

68
Q

What does the R ( universal gas constant describe?

A

Relationship between temperature and kinetic energy.

69
Q

T/F: Non-reacting gaseous volume are additive?

A

True : AIR

70
Q

What is perfusion-limited gas exchange?

A

The rate at which gas is transported away from functioning alveoli and into tissues is principally limited by the rate of blood flow through the pulmonary capillaries and this across the alveolar membrane.

71
Q

T/F: Idea gases do exist

A

False

72
Q

What does the Joule’s Thompson effect state?

A

A thermodynamic process that occurs when a fluid expands from high pressure to low pressure at constant enthalpy. -> as a cylinder of compressed gas empties, the cylinder cools.

73
Q

Whose law takes into consideration the that gases deviate form the ideal gas laws at high pressures and/or low temperatures.

A

Gander Waals Relationship

74
Q

What does relative humidity measure?

A

The saturation of water in the air

RH= mass of water that is in the air/ mass of water that will fill the air

75
Q

Dissolved CO2 in the blood is

A

0.067ml/100ml/mmHg partial pressure of CO2

GNUS561- Chem & Physics (2 decks)

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