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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
Diffusion of gases across a biological membrane is expressed by
Fick's Law
26
Fick's law states that
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.
27
Clinical Application of Fick's Law (5)
Allows determination of pulmonary gas exchange Diffusion Hypoxia COPD - reduced alveolar surface tension, slower induction Placental Drug Transfer 2nd gas effect
28
Diffusion Hypoxia
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
29
1 torr
1 torr = 1 mmHg
30
1 kPa
10.2 cm H2O = 7.5 mmHg/7.5 torr
31
1 atm =
760 mmHg = 1 bar = 14.7 PSI = 1020 cmH20
32
Compared to the volume of nitrogen diffusing out
the volume of nitrogen diffusing in is greater
33
Boyle's Law =
P1V1 = P2V2
34
with Boyle's Law, the volume is
inversely proportional to the pressure As pressure increases, volume decreases
35
Charles' Law =
V1/T1 = V2/T2
36
Charle's law states that
When pressure and n are constant, increase in volume is directly proportion to increase in temperature
37
Gay-Lussac's Law
P1 / T1 = P2/T2
38
Gay - Lussac's Law states
when volume is held constant, an increase in pressure is directly proportional to an increase in temperature.
39
Avogadro's #
6.022 e 23
40
If you have two different containers of two different gases as the same temperature and pressure then you can assume
they contain the same number of molecules.
41
Calibration of vaporizes is done using
Avogadro's Hypothesis
42
Dalton's Law
The total pressure of a gas mixture is the sum of the partial pressure of each gas
43
Critical temperature of oxygen
-119 celcius
44
Critical temperature of nitrogen
~ 36.5 - 39.5 celcius
45
Poisueille's Law describes
the relationship between rate of flow and pressure gradient, (direct) radius^4 of tube,(direct) length of tube,(inverse) viscosity. (inverse)
46
Applications of Poisueille's Law (4)
IV flows (blood) Airways (ex. heliox) Vascular flow - (anemia vs polycythemia) thorpe tubes (at low flows) hence laminar flow
47
Poisueille's law is applied with
LAMINAR flow
48
Factor will have the most dramatic effect on flow according to Poisueille's law
radius of tube
49
viscosity is
the inherent property of a fluid that resists flow
50
Reynold's number determines
laminar vs turbulent flow. >2000 = turbulent <2000 = laminar
51
Reynold's Number Equation
(velocity) x (density) x (diameter) // viscosity
52
Factors that change flow from laminar to turbulent
- increased velocity - bend >20 degrees - irregularity in the tube
53
turbulent flow often occurs in (airways)
medium to large airways, predominates phonation, coughing, peak flow
54
Smaller bronchioles can maintain
laminar flow
55
Reynolds number is an index that incorporates
Poiuselles law and density
56
Reynolds number is directly proportional to
velocity, density, diameter
57
Reynolds number is inversely proportional to
viscosity
58
Reynolds number application:
Heliox. Has a much lower density than nitrogen helps restore laminar flow to constricted airways
59
Bernoulli's Theorem relates
pressure and velocity Increased velocity = decreased pressure. Therefore narrow diameter = increased velocity = decreased pressure
60
Venturi Effect
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
Clinical Applications of Bernoulli and Venturi
Nebulizers Venturi Masks Jet Ventilation
62
With Venturi effect air/gas are entrained
Air may be entrained into a flow of liquid, | or a liquid may be entrained into the flow of a gas.
63
Conada effect explains
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
La of LaPlace formula
tube = Tension = Pressure x radius sphere = 2Tension = Pressure x Radius
65
La of Laplace relates
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
La Place's law directly applies to alveoli in the absence
of surfactant
67
without surfactant, small alveoli
would collapse as they would require higher pressure to open compared with larger alveoli
68
Surfactant Lowers the surface tension more in
smaller alveoli r/t having a more concentrated effect
69
Applications of La Place's Law
alveoli + surfactant vascular pathology (aneurysms) ventricular volume and work of the heart
70
Clinical applications of Ohm's LAw
strain gauges in pressure transducers | thermistors
71
Aneursyms are more likely to rupture because
they will have a greater tension along the part with a wider radius compared to the rest of the vessel
72
1 dyne =
force required to move 1 g of weight 1 cm per second
73
osmotic pressure vs oncotic presssure
oncotic pressure = osmotic pressure exerted by a plasma protein osmotic pressure = force needed to stop osmosis from occurring.
74
Reynolds number equation
velocity x density x diameter / viscosity

gtown nur641 (7 decks)

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