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gtown nur641 > ChemPhys Review > Flashcards

ChemPhys Review Flashcards

1
Q

Molecular Theory of Matter

A

states that matter is made of minute particles called molecules, that exist in various states (solid, liquid, gas, or plasma)

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2
Q

Kinetic Theory of Matter

A

states that molecules are in constant motion (random motion) and have a degree of attraction between them called van der waals forces.

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3
Q

Critical Temperature

A

the temp. above which a gas cannot be liquefied regardless of how much pressure is applied

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4
Q

Liquid; compressability

A

Liquids have minimal to no compressibility, volume MAY change with change in pressure or temperature

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5
Q

Gases; compressability

A

Gases are easily compressible

Easily change volume with changes in pressure or temperature

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6
Q

Structural Isomers

A

Have the same molecular formula, but their atoms are located in different places.

Structural isomers are truly different molecules with differing physical and chemical properties

(Enflurane and isoflurane are examples of structural isomers)

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7
Q

Stereoisomers

A

molecules that have a similar geometric arrangement of atoms but differ in their spatial position.

may be enantiomers or diastereomers .

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8
Q

Enantiomers

A

Stereoisomers that are mirror images of each other but cannot be super imposed.

Possess similar chemical, physical properties.

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9
Q

Enantiomers are optically

A

active, can rotate light either clock wise or counter clockwise.

Clockwise = dextro
Counter clockwise = levo

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10
Q

Diasteromers

A

are not mirror images, and may have differing physical and chemical properties.

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11
Q

In liquids, gas solubility is inversely related to

A

temperature

As temperature increases, LESS gas is dissolved in a liquid.

R/t increased kinetic energy of gas molecules.

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12
Q

Hypothermic patients and emergence

A

Hypothermic patients have a slower emergence r/t their decreased body temperature.

Colder temp = more gas is able to dissolve in blood.

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13
Q

Gas solubility in a liquid is directly related to

A

Pressure.

Henry’s law, more pressure = greater solubility of gases in liquids

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14
Q

Henry’s Law states

A

At a constant temperature, the amount of gas dissolved in a liquid is directly proportional to the partial pressure of the gas in contact with the solution`

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15
Q

Henry’s law allows calculation of

A

dissolved O2 and CO2 in blood

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16
Q

Formula for deriving oxygen content in blood

A

PaO2 X solubility co-efficient

PaO2 x 0.0031

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17
Q

Formula for deriving oxygen contenting blood

A

PCo2 x solubility co-efficient

PCo2 x 0.067

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18
Q

Formula for oxygen delivery

A

DO2 = CO x (1.34 X SaO2 x hgb) + (PaO2 x 0.0031) x 10

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19
Q

Overpressuring:

A

increase the concentration set on the vaporizer of pressure of gas to speed up delivery to the blood and, therefore, the brain

Application of Henry’s Law

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20
Q

Graham’s Law

A

A gas diffuses at a rate that is inversely proportion to the square root of its molecular weight

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21
Q

As molecular weight increases, diffusion

A

decreases.

As molecular weight increases the rate of diffusion decreases.

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22
Q

Smaller molecules diffuse

A

faster

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23
Q

nitrous oxide is contraindicated in patients with

A

pneumothorax,
or another air filled cavity where expansion is undesirable.

ex. abdominal surgery.

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24
Q

Diffusion

A

the net movement of one type of molecule through space as a result of random motion to minimize a concentration gradient

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25
Q

Diffusion of gases across a biological membrane is expressed by

A

Fick’s Law

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26
Q

Fick’s law states that

A

diffusion of a gas across a semipermeable membrane is directly proportional to the partial pressure gradient, the membrane solubility of the gas, and the membrane area, and is inversely proportional to the membrane thickness and the molecular weight of the gas.

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27
Q

Clinical Application of Fick’s Law (5)

A

Allows determination of pulmonary gas exchange

Diffusion Hypoxia

COPD - reduced alveolar surface tension, slower induction

Placental Drug Transfer

2nd gas effect

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28
Q

Diffusion Hypoxia

A

During emergence from nitrous oxide anesthetic, rapid elimination of nitrous oxide from the lungs dilutes other alveolar gases, producing alveolar “diffusion hypoxia.” This phenomenon is driven by the same mechanism as the second gas effect—but in the reverse direction

too much nitrogen being exhaled, dilutes other gases, leads to hypoxia

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29
Q

1 torr

A

1 torr = 1 mmHg

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30
Q

1 kPa

A

10.2 cm H2O = 7.5 mmHg/7.5 torr

31
Q

1 atm =

A

760 mmHg = 1 bar = 14.7 PSI = 1020 cmH20

32
Q

Compared to the volume of nitrogen diffusing out

A

the volume of nitrogen diffusing in is greater

33
Q

Boyle’s Law =

A

P1V1 = P2V2

34
Q

with Boyle’s Law, the volume is

A

inversely proportional to the pressure

As pressure increases, volume decreases

35
Q

Charles’ Law =

A

V1/T1 = V2/T2

36
Q

Charle’s law states that

A

When pressure and n are constant, increase in volume is directly proportion to increase in temperature

37
Q

Gay-Lussac’s Law

A

P1 / T1 = P2/T2

38
Q

Gay - Lussac’s Law states

A

when volume is held constant, an increase in pressure is directly proportional to an increase in temperature.

39
Q

Avogadro’s #

A

6.022 e 23

40
Q

If you have two different containers of two different gases as the same temperature and pressure then you can assume

A

they contain the same number of molecules.

41
Q

Calibration of vaporizes is done using

A

Avogadro’s Hypothesis

42
Q

Dalton’s Law

A

The total pressure of a gas mixture is the sum of the partial pressure of each gas

43
Q

Critical temperature of oxygen

A

-119 celcius

44
Q

Critical temperature of nitrogen

A

~ 36.5 - 39.5 celcius

45
Q

Poisueille’s Law describes

A

the relationship between rate of flow and

pressure gradient, (direct)
radius^4 of tube,(direct)
length of tube,(inverse)
viscosity. (inverse)

46
Q

Applications of Poisueille’s Law (4)

A

IV flows (blood)
Airways (ex. heliox)
Vascular flow - (anemia vs polycythemia)
thorpe tubes (at low flows) hence laminar flow

47
Q

Poisueille’s law is applied with

A

LAMINAR flow

48
Q

Factor will have the most dramatic effect on flow according to Poisueille’s law

A

radius of tube

49
Q

viscosity is

A

the inherent property of a fluid that resists flow

50
Q

Reynold’s number determines

A

laminar vs turbulent flow.

> 2000 = turbulent

<2000 = laminar

51
Q

Reynold’s Number Equation

A

(velocity) x (density) x (diameter) // viscosity

52
Q

Factors that change flow from laminar to turbulent

A
  • increased velocity
  • bend >20 degrees
  • irregularity in the tube
53
Q

turbulent flow often occurs in (airways)

A

medium to large airways, predominates phonation, coughing, peak flow

54
Q

Smaller bronchioles can maintain

A

laminar flow

55
Q

Reynolds number is an index that incorporates

A

Poiuselles law and density

56
Q

Reynolds number is directly proportional to

A

velocity, density, diameter

57
Q

Reynolds number is inversely proportional to

A

viscosity

58
Q

Reynolds number application:

A

Heliox. Has a much lower density than nitrogen helps restore laminar flow to constricted airways

59
Q

Bernoulli’s Theorem relates

A

pressure and velocity

Increased velocity = decreased pressure.
Therefore narrow diameter = increased velocity = decreased pressure

60
Q

Venturi Effect

A

The lateral pressure of rapidly flowing fluid in a constricted tube can be sub-atmospheric, hence a sidearm on that portion of the tube can be used to aspirate another fluid into the tube

61
Q

Clinical Applications of Bernoulli and Venturi

A

Nebulizers
Venturi Masks
Jet Ventilation

62
Q

With Venturi effect air/gas are entrained

A

Air may be entrained into a flow of liquid,

or a liquid may be entrained into the flow of a gas.

63
Q

Conada effect explains

A

tendency of fluid flow to follow a curved surface upon emerging from a constriction.

will choose the path that is slower to return to increased pressure.

64
Q

La of LaPlace formula

A

tube = Tension = Pressure x radius

sphere = 2Tension = Pressure x Radius

65
Q

La of Laplace relates

A

Pressure gradient across the wall of a SPHERE or TUBE/CYLINDER (blood vessel, ventricle, alveolus) is directly related to tension and
inversely related to radius

66
Q

La Place’s law directly applies to alveoli in the absence

A

of surfactant

67
Q

without surfactant, small alveoli

A

would collapse as they would require higher pressure to open compared with larger alveoli

68
Q

Surfactant Lowers the surface tension more in

A

smaller alveoli r/t having a more concentrated effect

69
Q

Applications of La Place’s Law

A

alveoli + surfactant
vascular pathology (aneurysms)
ventricular volume and work of the heart

70
Q

Clinical applications of Ohm’s LAw

A

strain gauges in pressure transducers

thermistors

71
Q

Aneursyms are more likely to rupture because

A

they will have a greater tension along the part with a wider radius compared to the rest of the vessel

72
Q

1 dyne =

A

force required to move 1 g of weight 1 cm per second

73
Q

osmotic pressure vs oncotic presssure

A

oncotic pressure = osmotic pressure exerted by a plasma protein

osmotic pressure = force needed to stop osmosis from occurring.

74
Q

Reynolds number equation

A

velocity x density x diameter / viscosity

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