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Chem/ Phys > Physics/ Math > Flashcards

Physics/ Math Flashcards

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1
Q

Molecular Theory of Matter

A

Matter is made of minute particles called molecules, that exist in various states (s, l, g)

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2
Q

Kinetic Theory of Matter

A

Molecules are in constant (random) motion and have a degree of attraction b/w them called van der waals forces

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3
Q

Critical Temperature

A

temp, above which, a gas cannot be liquified regardless of how much pressure is applied

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4
Q

Avogadro’s Hypothesis

A

if you had 2 different containers containing 2 different gases (@ the same T and P), they contain the same # of mlcs

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5
Q

Avogadro’s Number

A

1 mole = 6.02 x 10^23 mlcs
1 mol = 1g x molecular wt
1 mol of any substance = 22.4 L

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6
Q

Avogadro & anesthesia

A 
Calibration of vaporizers uses
Sevo mlc wt = 200g = 1 mole 
   so occupy 22.4L @STP
20g of sevo = .1 mol into vaporizer, 
  should occupy  2.24 L
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7
Q

Boyle’s Law

A 
Constant = PV (k1)
P & V relationship, 
T contant
V = 1/P
Vol of ideal gas inverse proportional to P
   Ex: Reservoir Bag
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8
Q

Universal Gas Constant

A

PV/T = constant (k4) for gas

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9
Q

Applying Boyle’s Law

A

Full E cylinder of O2 will empty large vol into atmosphere 625-650L (low P = high Vol)
Spontaneous breathing
Bellow in Vent

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10
Q

Charles’ Law

A

V proportional to T
P stay constant
V/T = constant
Ex: Tec 6, balloon bust on hot day

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11
Q

Guy-Lussac’s Law

A

P and T proportional
V constant
EX: gas cylinder full & moved to hot room

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12
Q

Universal Gas Law

A

PV = nRT

EX: cylinder P decreases as gas empties, mol decreases too

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13
Q

Dalton’s Law

A

Total P of gas mix is sum of the partial Ps of each gas

Pressure exerted by each gas is same as if it was alone in container

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14
Q

Fick’s Law

A 
Rate of diffusion of substance across membrane r/t:
  Directly by: 
1) Concentration gradient
2) SA of membrane
3) Solubility
   Inversely by:
4) thickness of membrane
5) Molecular Wt

Vgas = Area x Solubility x PP diff
/ Mlc Wt x Distance

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15
Q

Ficks Application

A

2nd Gas Effect:
high inspired concentration of 1st gas (N2O) accelerates uptake of companion gas

Concentration Effect: high vol of N2O concentrates remaining 2nd gas

Diffusion Hypoxia: Diffusion of gas across alveolo-capilary membrane

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16
Q

Ficks Application 2

A

Expansion of Air Pockets
-N2O 34x more soluble in blood than N2 =
>Vol N2O diffusing in than N2 Vol out

Expansion of ET cuff w/ N2O in use

Placental transfer of drugs & O2

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17
Q

Graham’s Law

A

Gas diffuses at rate inversely proportional to square root of its mlc wt
> ml wt = < diffusion rate

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18
Q

Henry’s Law

A

Amount of gas dissolved in liquid directly proportional to partial P of gas in contact w the solution

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19
Q

Application of Henry’s Law

A

Calculate O2 & CO2 dissolved in blood
Constants:
O2: .003ml/100ml blood/ mmHg partial pressure
CO2: .067 ml/100ml blood / mmHg partial pressure

Multiply PaO2 x constant to get mls in 100mls of blood

Multiply FiO2 by 5 to get mm Hg, then multiply by .003 to get mls in 100mls of blood

20
Q

Critical Temperature

A

Temp above which a substance goes into gaseous form in spite of how much pressure is applied
If temp > critical temp can’t liquify gas

21
Q

Critical Temp of O2

A

-119 degree C
so can’t liquify @ room temp
-keep main hospital O2 supply @ -160 degrees C as liquid

22
Q

Critical Temp of N2O

A

39.5 degrees C

P can liquefy N2O @ room temp (25 C)

23
Q

Adiabatic Cooling

A

occur when matter changes phase
Change in temp of matter w/o gain/loss of heat
-frost forms d/t cooling when N2O opened fully

24
Q

Joule Thompson Effect

A

Expansion of a gas causes cooling

-gas leave cylinder, expansion cools air = condensation

25
Q

Poiseuille’s Law

& laminar flow

A

Describe relationship b/w rate of flow and:
DIRECT:
1) Pressure gradient across length of tube
2) radius^4 of the tube
INVERSE
3) length of the tube
4) viscosity of fluid

26
Q

Applications of Poiseuille’s Law

A

IV Flow,
Airways
Vascular Flow
Thorpe Tubes (@ low flowso

27
Q

Determinate of flow when:
low flow rates-
high flow rates

A

Low flow rate determinant is viscosity

High flow rates (turbulent gas) determined by density (heliox)

28
Q

Reynold’s Number

A

Reynold’s # = velocity * density * diameter
/ viscosity

R# >2000 = Turbulent flow

29
Q

Thorpe Tube

A

Low flow = annular orifice around float is tubular so flow determined by viscosity

High flow = annular opening more like orifice & density governs flow

30
Q

3 Factors that change flow from

Laminar –> Turbulent

A

1) > Velocity
2) Bend >20 degrees
3) Irregularity in the tube

31
Q

Bernoulli’s Theorem

A

Relate P & velocity
-Lateral wall P is least @ point of:
greatest constriction & speed
=faster flow

32
Q

Bernoulli’s Theorem

Narrow Diameter =

A

Small diameter =

< Lateral wall P = > speed

33
Q

Bernoulli’s Theorem

Wider Diameter =

A

Wider Diameter =

> Lateral Wall P = < speed

34
Q

Venturi Tube

A

application of Bernoulli’s

  • as tube narrows, velocity increases thus dropping the pressure
  • so we can find velocity by measuring pressure
35
Q

Clinical Applications of

Bernouilli and Venturi

A

Nebulizers
Venturi Oxgen Masks (20-40% O2)
Jet Ventilation

Lateral P of rapidly flowing fluid in constricted tube can be sub-atmospheric, so
Side arm on that part of tube can be used to aspirate another fluid into the tube

36
Q

Beer’s Law

aka Beer-Lambert Law

A

absorption of radiation of a solution (of a given concentration and thickness) is same as 2x that of a solution w/ x2 thickness and 1/2 convcentration

Each layer of thickness absorbs an equal fraction of radiation that passes through it

37
Q

Beer’s Law

Clinical Applications

A 
Pulse Oximetry
-2 LEDs,
  -Red emit light @ 660nm
  -Infrared emit light @ 940nm
compares 2 types of light absoprbed &amp; calculates oxygen saturation
OxyHgb 940nm (IR light)
DeoxyHgb 660nm (Red Light)
38
Q

Errors in Pulse Oximetry (6)

A
  1. Artifact: low perf, ambient light, motion
  2. Alternate Species of Hgb
    Carboxyhgb: false high
    MethHgb: >85% false low, <85% false high
    HgbF and HgbS: No Effect
  3. Polycythemia: no effect
  4. Methylene & Isosulfan Blue
    false low
  5. Indocyanine Green & Indigo Carmine
    slight decrease
  6. Blue Nail Polish: false low
39
Q

Law of La Place

A

Pressure gradient across the wall of a sphere (alveolus) or tube/cylinder (blood vessel/ ventricle) is r/t to:

Wall Tension (T) directly
&
Radius (r) inversely

T=Pr

40
Q

La Place’s Law

Clinical Applications 3

A
  1. Normal alveoli & surfactant need during expiration
  2. Vascular Pathology:
    aneurysm rupture d/t > wall tension
  3. Ventricular vol & work of the heart
    dilated ventricle has >tension in wall
    Rise in end-diastolic pressure
41
Q

Ohm’s Law

A

Resistance which will allow 1 ampere of current to flow under influence of potential of 1 volt

W = Potential(volt)/current (amp)

E= IR

42
Q

Ohm’s Law 2

Clinical Application of

A
  • Strain gauges in pressure transducers

- Thermistors

43
Q

Electricity in the OR

4

A
  1. Burns from metal
    -metal bed, blood wet, electrical equipment = burns
  2. Macroshock
    current distributed througn body
    by faulty wiring, bad grounding
  3. Microshock
    current applied in or near heart
    by pacing wires, faulty equipment during cardiac cath
  4. Electrocautery
44
Q

Macroshock

A 
1 milliamp --> tingling/perception
5 --> max harmless current
10-20 milliamps --> let go
50 milliamps --> pain/LOC./ mech injury
100-300 milliamps --> V-fib, resp intact
6000 milliamps --> complete physiologic damage
45
Q

Microshock

A

50-100 microamps –> V-fib

46
Q

Percentage Solutions

A

grams per cent/100

2% Lidocaine = 2g in 100mls
or 20mg per ml

To get mg in 1 ml, move decimal to R x1 of the %

47
Q

Concentration Solutions

A

grams per x ccs
1:100,000 Epi =
1g per 100,000 cc

FYI: 1mg=1000mcg
1g = 1000mg

Chem/ Phys (8 decks)

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