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N927 Chem/Physics > 9 Gas Laws & Gas Cylinders > Flashcards

9 Gas Laws & Gas Cylinders Flashcards

1
Q

PAO2 Equation

A 
PAO2 = FiO2 x (PB - PH2O) - (PaCO2/RQ)
RQ = 0.8
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2
Q

Alveolar/Arterial Ratios

A

Alveolar-arterial oxygen difference/gradient
(A - a)DO2 or PAO2 - PaO2
Normal 5-15mmHg

Arterial-alveolar ratio
PaO2/PAO2
Normal > 0.75

PaO2/FiO2
Normal >200

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3
Q

Henry’s Law

A

Cgas = Pgas / KH

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4
Q

Dissolved PaO2

A

0.003ml O2 dissolved in 100ml blood per 1mmHg PO2 applied
PAO2 = 100mmHg
PaO2 = 0.3ml O2

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5
Q

Dissolved CO2

A

0.067ml CO2 dissolved in 100ml blood per 1mmHg PCO2

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6
Q

Arterial O2 Content Equation

A

CaO2 = ((1.34ml O2/gm Hgb) x (15gm Hgb/100ml blood) x (% saturation)) + (0.003 x PaO2)

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7
Q

O2 Delivery

A

= CaO2 content x CO

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8
Q

Boyle’s Law

A

Gas pressure inversely proportional to volume at constant temperature
P1 x V1 = P2 x V2

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9
Q

Charles’ Law

A

Gas volume directly proportional to absolute temperature (°K) at constant pressure
V1/T1 = V2/T2

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10
Q

Gay-Lussac’s Law

A

Gas pressure directly proportional to absolute temperature (°K) at constant volume
P1/T1 = P2/T2

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11
Q

Combined Gas Laws

A

(P1xV1)/T1 = (P2xV2)/T2

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12
Q

Avogadro’s Law

A

Equal gas volumes at same temperature and pressure contain the same number molecules or atoms
V1/n1 = V2/n2

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13
Q

Avogadro’s Number

A

1 mole gas @ STP = 6.02 x 10^23 molecules
GMW 1 mole O2 = 32g
2kg tank N2O (44g) = 45.45 Mole

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14
Q

1 Mole Gas = x L

A

22.4L @ STP

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15
Q

Ideal Gas Law

A 
Avogadro + Boyle + Charles + Dalton
PV/T = Rn
PV/nT = R
PV = nRT
V = nRT/P
R (constant) = 62.36 L⋅mmHg/Mol⋅K
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16
Q

Oxygen Tank

A

E tank

14.7psi / 5L
(PSI/14.7) x 5L
L/flow = min

Holds 660L
1900psig

17
Q

Nitrous Oxide Tank

A

Pressure gauge (psig) does not change until N2O unable to move from liquid to gas state (no liquid present)
Open valve → releases gas ↓pressure
Liquid N2O changes to gas state ↑pressure
Equilibrates on pressure gauge Ø change
*Weigh tank to determine N2O remaining
Able to hold more volume w/ less psi than E cylinder tank d/t ↑ Moles (liquid more dense than gas)
Mass N2O present / GMW (44g) = # Moles (n) N2O
V = nRT/P

Holds 1590L
745psig

18
Q

Joule-Thomson Effect

A

Decrease in temperature as heat loss result when gas expands freely into space
Compression & expansion
Normal conditions compression/expansion occurs slowly enough that heat transfer (exothermic/endothermic reactions) not felt of observed
Heat change dissipates into the environment

19
Q

Compression

A

Exothermic reaction
↑ kinetic energy when compressed
Heat lost to the environment
Anesthesia machine gas compression via narrow valve = heat
Ignition possible, especially in high O2 environment

20
Q

Expansion

A

Work requires energy (heat)
Endothermic reaction
Area surrounding rapidly expanding gas will feel cold
Gas cylinder release - cold regulator

21
Q

Adiabatic Compression/Expansion

A

Rapid compression (exothermic) heat liberation does not have time to dissipate
Things in vicinity or in contact w/ gas will heat up
Rapid expansion (endothermic) surrounding area will feel cold
OR insulated area where compression/expansion occurs ჻ heat trapped and unable to dissipate

22
Q

Concentration Effect

A

Accelerating alveolar gas concentration by increasing inspired concentration
Alveolar fraction (FA) / Inspired fraction (FI)
Optimal FA/FI ratio = 1
How quickly anesthetic gas enters bloodstream & crosses the blood-brain barrier
Patient who receives higher concentration will feel anesthetic effects sooner

23
Q

2nd Gas Effect

A

Large volume uptake (highly soluble) gas N2O delivered at high concentration to accelerate alveolar partial pressure increase of anesthetic (ex: Isoflurane)
Concurrent gas administered w/ anesthetic
Oxygen + anesthetic + nitrous oxide
N2O highly soluble and quickly absorbed into blood → leaves void in alveolus
Effect: Concentrates anesthetic gas & suctions in more gas from airways = ↑ anesthetic
Result: Able to anesthetize patient more quickly d/t ↑ anesthetic concentration in the alveolus

N927 Chem/Physics (12 decks)

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