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NU 724 - Chem/Phys > Exam III > Flashcards

Exam III Flashcards

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1
Q

Boyle’s Law

A

At a constant temperature, pressure and volume are inversely related.

P1 x V1 = P2 x V2

Ex. Ambubag

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2
Q

Dalton’s Law of Partial Pressures

A

The total pressure exerted by a gaseous mixture is equal to the sum of the partial pressures of each individual component in a gas mixture.

Pt = P1 + P2 + P3 …

Ex. Calculate the partial pressure of each gas in room air.

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3
Q

Avogadro’s Law

A

Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules.

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4
Q

Avogadro’s Numbers

A

1 mole of gas = 6.023 x 10^23 molecules

Molar volume of any ideal gas = 22.7 L at STP

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5
Q

Fick’s Law of Diffusion

A

Accounts for molecular weight, concentration gradient, solubility, and membrane interactions (surface area and thickness).

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6
Q

Diffusion is directly proportional too… (3)

A

Difference in partial pressure

Area of the membrane

Solubility of the solute

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7
Q

Diffusion is inversely related to… (2)

A

Thickness of the membrane

Square root of the molecular weight

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8
Q

Graham’s Law of Effusion

A

The rate of effusion (gas moving through a small orifice) of a gas is inversely proportional to the square root of its molecular weight.

Ex. CO2 and O2 (CO2 is more soluble, but a larger molecule).

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9
Q

Henry’s Law

A

At a constant temperature, the amount of gas dissolved in a liquid is directly proportional to the partial pressure of the gas in equilibrium with the liquid.

If we increase the partial pressure of a gas above a liquid, we will also increase the partial pressure of the same gas in the liquid.

p = kc

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10
Q

Ideal Gas Law/Universal Gas Law

A

Combines Boyle’s, Charles’, Gay-Lussac’s and Avogadro’s laws.

Allows us to calculate the volume for which 1 mole of a gas will expand at any given temperature or pressure.

Can be used to calculate precisely how much O2 is left in a cylinder.

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11
Q

Ideal Gas Law/Universal Gas Law Equation

A

P x V = n x R x T

P = Pressure
V = Volume
n = # of moles
R = Gas constant (0.0821 Latm/molk)
T = Temperature (kelvin)

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12
Q

Gas Constant

A

0.0821 Latm/molk

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13
Q

Molecular Weight of N2O

A

44g

Atomic weight:
N = 14
O = 16

14 + 14 + 16 = 44

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14
Q

Molecular Weight of O2

A

32

Atomic weight:
O = 16

16 + 16 = 32

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15
Q

Celsius to Kelvin

A

K = C + 273.15

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16
Q

Fahrenheit to Celsius

A

(F - 32) x 5/9 = C

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17
Q

Concentration Effect

A

N2O is 35x more soluble in blood than N
→ rapid movement of N2O across lung tissue into the blood and slow replacement of N from blood into the alveoli
→ net movement of molecules out of alveoli causes them to shrink
→ gases left behind are therefore concentrated in a smaller space.

*Boyle’s Law + Fick’s law

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18
Q

Second Gas Effect

A

Volatile agent + N2O
→ N2O rapidly diffuses
→ concentration of volatile agent increases
→ creates a larger pressure gradient from the alveoli into the blood
→ higher rate of diffusion.

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19
Q

Diffusion Hypoxia

A

Body tissue is saturated with N2O at the end of surgery.

If we do not allow enough time to replace N2O with O2 during emergence, the rapid influx of N2O into the alveoli will dilute the partial pressure of O2 in the alveoli.

If patient is placed on RA instead of 100% FiO2, the dilution of oxygen will be equal to breathing a hypoxic gas mix.

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20
Q

N2O Tank Calculations (>745 psi)

A

Utilize ideal gas law:
V = (n x R x T) / P

Ex. N2O tank has 2000g left (Current weight - tare weight)

2000g / 44 g/mole = 45.22 moles

V = (45.22 x 0.0821x 298) / 1 atm = 1111.7 L

Flow rate @ 2L / min

1111.7 L / 2 L /min = 555.85 mins / 60 = ~9.26 hours.

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21
Q

N2O Tank Calculations (<745 psi)

A

V2 = (V1 x P2) / P1

Ex. 1/4 tank = 250 L/745psi Tank psi = 620 psi

V2 = (250 x 620) / 745 = 208 L

Flow rate: 7 L / min = 208 / 7 = 29.71 mins = ~30 mins

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22
Q

O2 Tank Calculations

A

V2 = (V1 x P2) / P1

Ex. Full O2 tank = 660L/2200 psig. Tank reads 620 psig and O2 flow @ 4 L/min

V2 = (660 x 620) / 2200 = 186L / 4 = 46.5 mins

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23
Q

Vapor Pressure

A

Pressure exerted by the molecules of a liquid that have been liberated to a vapor form on the walls of a closed container at thermodynamic equilibrium.

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24
Q

Saturated Vapor Pressure (SVP)

A

Amount of pressure exerted by the vapor at equilibrium with its condensed state at a specific temperature.

The amount of pressure a vapor can exert before it returns to its liquid state.

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25
Q

Altitude

A

Increased altitude will increase anesthetic gas concentration.

Decreased altitude will decrease anesthetic gas concentration.

Anesthetic depth is dependent on partial pressure of anesthetic gas.

When atmospheric pressure decreases (increased altitude), liquids boil at lower temperatures.

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26
Q

Desflurane Vapor Pressure

A

669 mmHg

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27
Q

Isoflurane Vapor Pressure

A

238 mmHg

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28
Q

Sevoflurane Vapor Pressure

A

137 mmHg

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29
Q

Incorrect Volatile Agent in Vaporizer

A

High (VP) → Low (Vaporizer) → High (Dose)

Low (VP) → High (Vaporizer) → Low (Dose)

Ex. Sevo (137) → Iso Vaporizer (238) → Low dose

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30
Q

Boiling Point

A

Temperature the bulk of the liquid at a given pressure converts to vapor.

Occurs when the vapor pressure is greater than or equal to atmospheric pressure.

Decreased atmospheric pressure = Decreased boiling point

Ex. The higher the VP (at room temp), the lower the boiling point (Desflurane).

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31
Q

Partial Pressure

A

The pressure of an individual component in a gaseous mixture.

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32
Q

Solids

A

Materials that resist change in shape and volume

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33
Q

Liquids

A

Fluids that exhibit minimal to no compressibility and may change volume with changes in pressure and temperature.

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34
Q

Gases

A

Fluids that are compressible and easily change volume with changes in pressure and temperature.

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35
Q

Melting

A

Solid → Liquid

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36
Q

Evaporation

A

Liquid → Gas

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37
Q

Condensation

A

Gas → Liquid

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38
Q

Freezing

A

Liquid → Solid

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39
Q

Sublimation

A

Solid → Gas

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40
Q

Deposition

A

Gas → Solid

41
Q

Critical Temperature

A

Temperature above which a substance can no longer be liquefied by the application of pressure alone.

> Critical temp → gas
< Critical temp → vapor (exists in equilibrium with the liquid phase).

42
Q

Critical Pressure

A

Pressure required to liquefy a vapor at its critical temperature.

43
Q

Heat of Fusion (enthalpy of fusion)

A

Amount of energy required to change a substance from a solid state to a liquid state at a constant temperature and pressure.

Occurs at the melting point.

44
Q

Heat of Vaporization (enthalpy of vaporization)

A

Amount of heat energy required to change a substance from a liquid state to a gaseous state at a constant temperature and pressure.

Occurs at boiling point.

45
Q

Law of Laplace

A

Relationship between pressure, radius, and tension in a spherical or cylindrical shape.

46
Q

Law of Laplace: Cylinder

A

T = P x r

Tension is directly proportional to pressure and radius.

Radius increases → pressure decreases.
Radius decreases → pressure increases.
If radius and pressure increase → Tension increases

Ex. Blood vessels

47
Q

Law of Laplace: Sphere

A

2T = P x r OR T = P x (r/2)

Spheres can handle x3 the pressure or radius.

48
Q

Law Used to Calculate O2 Tanks

A

Boyle’s Law: V1 + P1 = V2 + P2
or
V2 = (V1 - P2) / P1

49
Q

Coulomb’s Law

A

The change in potential energy caused by the movement of electrons from an area of high concentration or high charge density to an area of low concentration or low charge density.

Like charges repel.

Opposite charges attract.

50
Q

Coulomb

A

SI unit for electric charge

The amount of electrical charge transported in one second by a steady current of one ampere.

51
Q

Ohm’s Law

A

Potential flow of electrical charge is proportional to actual current after accounting for resistance.

V (voltage) = A (current) x O (resistance)

Ex. BP = CO x SVR

52
Q

Current

A

How much charge is flowing past a point in a circuit in 1 second

Coulomb/sec or amperes (amps)

53
Q

Beer Lambert’s Law

A

Lambert’s = Intensity of transmitted light decreases as the distance travelled through the substance increases.

Beer’s = Intensity of transmitted light decreases as the concentration of the substance increases.

54
Q

Pulse Oximetry

A

Applies to Beer-Lambert law to the absorption of two specific frequencies (infrared and visible red) by hemoglobin.

55
Q

Visible Red Wavelength

A

Absorbed by DEOXYgenated hemoglobin.

660nm

56
Q

Infrared Wavelength

A

Absorbed by OXYgenated hemoglobin.

940 nm

57
Q

Disadvantages of Pulse Oximetry (6)

A

Susceptible to artifact and light.

Limits with hypothermic or vasoconstricted states.

Nail polish/acrylics.

Dye interference (ICG and methylene blue).

Abnormal hgb states and erroneous values (carbon monoxide).

Risk of burns in poor perfusion states.

58
Q

Causes of Electrical Injury

A

Direct contact with metal casing due to insulation damage or faulty construction.

Inductance due to the magnetic field of alternating current, producing a small electrical flow in the surrounding metal casing despite no direct contact.

Stray capacitance from buildup of electrical potentials with with an alternating current circuit despite no closed-circuit electrical flow.

59
Q

Macroshock

A

Electrical shocks that traverse intact skin.

Larger amounts of current applied to the external surface of the body.

The impedance of the skin offers a higher resistance which requires a greater current to induce vfib.

60
Q

DC Circuit

A

Direct current flow of electrons in one direction

61
Q

AC Circuit

A

Alternating circuit

Flow of electrons reverses direction @ set frequency (60 Hz)

62
Q

Line Isolation Monitor (LIM)

A

Device placed between the live wires and the ground to measure the impedance to flow.

Alarms if a live wire has contact or high capacitance to ground.

63
Q

LIM Alarms Protocol

A

Alarms @ 2-5 mA

Disconnect last piece of equipment plugged into and inspect it to verify that it is the offending item.

May also be activate because of the cumulative effect of minor leakage of many piece of properly working equipment but no risk present.

64
Q

Microshock

A

Smaller amounts of current that is applied directly to the myocardium.

Since skin is bypassed, it takes much less current to induce vfib.

65
Q

What increases susceptibility to microshock?

A

Direct pathways:
CIV
PA catheters
Pacer wires

66
Q

Macroshock threshold for perception

A

1 mA

67
Q

Macroshock for Loss of Consciousness

A

50 mA

68
Q

Macroshock for Vfib

A

100-300 mA

69
Q

Microshock for Vfib

A

100 μA

70
Q

Power units

A

Watts

71
Q

Electrical potential units

A

Volts

72
Q

Electrocautery

A

High frequency electrical currents to cauterize, cut, and destroy tissue,

73
Q

Bipolar Devices

A

Two tips

One to supply the electrical current and the other to return the current.

Does not require a return electrode.

Less likely to cause burns or injuries apart from local area of use.

74
Q

Unipolar Device

A

One tip

To deliver electrical current, large surface area return electrode with good conductive contact must be place on the patient (grounding pad).

Path of current flow to the ground pad must not cross the patients heart.

75
Q

Considerations with Electrocautery

A

ECG → Artifact

Pacemakers → May sense electromagnetic conductance as inherent electrical activity and not pace

Magnet → Place on PPM to fire at asynchronous rate (ALWAYS interrogate PPM as part of pre-op assessment).

76
Q

How does EMR interact with matter?

A

Reflected

Refracted (Scatter)

Diffracted (Redirected)

Absorbed (Interfered)

77
Q

Radiation Safety

A

Time → Minimize
Distance → 6 feet away
Shielding → Lead

78
Q

Max Dose of Radiation

A

5 rems / 5,000 milirems

79
Q

Ionizing Radiation

A

Radiation capable of ionizing → the removal of an electron from an atom.

Ionizing radiation is so named because it is capable of removing an orbital electron from matter.

Causes cellular injury.

80
Q

Examples of Ionizing Radiation

A

X rays
Gamma rays
Alpha and Beta particles

81
Q

Non-ionizing Radiation

A

Radiation for which the mechanism of action in tissue does not involve ionization.

82
Q

Examples of Nonionizing Radiation

A

Visible light
Infrared radiation
Microwaves
Radio-waves
MRI
Ultrasound

83
Q

LASER

A

Light amplification by stimulated emmision of radiation.

84
Q

Function of Lasers

A

They use a continual energizing of atoms in order to force photons that are of the same frequency and direction to be released which results in continuous production of monochromatic and unidirectional photons which can be directed into a laser beam.

85
Q

Types of Lasers

A

CO2
Nd:YAG
Argon
Ruby

86
Q

CO2 Laser Uses

A

Head, neck, face surgery
Airway surgeries

Longer wavelength, does not penetrate as deep into tissue
More suitable for superficial lesions or airway surgeries

87
Q

Nd:YAG Laser Uses

A

Generalized cutting and coagulation

Shorter wavelength, greater ability to penetrate and destroy tissues.

88
Q

Argon Laser Uses

A

Vascular lesions

89
Q

Ruby Laser Uses

A

Retinal surgery

90
Q

Laser Safety Considerations

A

Ignition source in presence of oxygen.

Eye protection for staff and patient

Smoke precautions

Misdirected beam

91
Q

ETT Fire Protocol (8 steps)

A

Stop O2 flow
Stop ventilation
Disconnect circuit
Extubate patient
Extinguish fire
Mask ventilate
Reintubate
Refer for bronch, lavage, steriods

92
Q

ETT Fire Prevention

A

Use low FiO2

Use nonflammable or shielded ETT cuff

Saline + methlyene blue in ETT cuff

Saline/sterile water on standby

93
Q

Charge SI Unit

A

Coulombs (C)

94
Q

Electrical Potential SI Unit

A

Volts (V)

95
Q

Current SI Unit

A

Amperes (A)

96
Q

Resistance SI Unit

A

Ohms (Omega)

97
Q

Power SI Unit

A

Watts (W)

98
Q

How do lasers function? (4)

A

Population inversion

Stimulated Emission

Stimulated Absorption

Spontaneous Emissions

99
Q

How doe lasers differ from light? (3)

A

Monochromatic

Spatial Coherences

Collimation

NU 724 - Chem/Phys (3 decks)

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