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Pr. Konstantin M. LEBEDINSKY
Course : 1
Year : 2009
Language : EnglishCountry : Estonia
City : Tartu
Weight : 3624 kb
Related text : no http://www.euroviane.net
THE PHYSICAL LAWS, ESSENTIAL
FOR THE ANAESTHETIST
St. Petersburg
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Matter
Substance Field
States of matter:
Solid
Liquid
Gas
Plasma
• Electric
• Magnetic
• Gravitational• Torsion
• Biological
• Informational
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«Primary» Physical Values
(Mechanics)
• Mass М kg
• Length L m
• Time t s
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Derivative Physical Values
(Mechanics)• Velocity v Lt-1 m/s
• Acceleration a Lt-2 m/s2
• Force F MLt-2 N = kgm/s2
• Pressure P ML-1
t-2
Pa = N/m2
• Energy (work) E(A) ML2t-2 J = Nm
• Power N ML2t-3 W = J/s
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What is Power of a Pump?…What are we to do to get Power (ML2
t-3)?
We suppose, that it depends upon Pressure(ML-1t-2). Let’s divide Power by Pressure:
ML2t-3 /ML-1t-2 = L3t-1
Since m3 /s is Flow, for any kind of the pump –Power is Pressure multiplied by Flow :
N = PQ!
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Pressure Units
• Pa = N/m2
• cm Н2О 100 Pа = 0,1 к Pа = 1 hPа
• atm 10 m Н2О 100.000 Pа = bar
• mbar = 100 Pа 1 cm Н2О
• mm Hg = torr = 133,3 Pа
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Gas Laws
Boyle’s Law (1661):Condition: T=const (isotermic)
PV = const or P1 /P2 = V2 /V1
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Gas Laws
Charles’ Law (1787):Condition: V=const (isovolumic)
P/T = const or P1 /Р2 = T1 /Т2
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Gay-Lussac’s Law (1809):Condition: P=const (isobaric)
V/T = const or V1 /V2 = T1 /Т2
Gas Laws
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Th. Andrew’s
isothermals (1869)
Boyle’s law: since T=const, PV = const
Charles’ law: since V=const, P /Т = const
Gay-Lussac’s law: since P=const, V/T = const
Hereby,
the equation of an ideal gas:
PV/T = const
or PV = mRT
P
V
T
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Critical Temperature –
the temperature above which a gas cannot be liquefied no
matter how high the pressure (marked with bend point onthe isothermals). Critical temperature corresponds withcritical volume and critical pressure, above which liquid andgas coexists in the equilibrium.
Tcrit values, С:
Helium –268 Carbon Dioxide 31
Oxygen –118 Nitrous Oxide 36
Nitrogen –147 Xenon 17
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Compressed Gases
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Liquefied Gases
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What gas is it?
!
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Where is Oxygen Cylinders?
http://www.made-in-jiangsu.com/
!
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Oxygen Sources
• Pressure cylinders with pressure-regulating valves• Centralized systems with cryogenic reservoirs
• «Oxygen Concentrators» and Zeolite-based systems
• O2-flush requirements: 4…5 atm for the input!
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Dalton’s Law (1801):
The total pressure exerted by the mixture of gases, which
do not interact, is the sum of the pressures which eachgas would exert if it were present alone in the entire
volume occupied by the mixture (i.e. partial pressures).
Partial pressure reflects the number of molecules and its
kinetic energy, depending upon the fraction of certaingas in the mixture (%) and the pressure of the entire
mixture, respectively:
PX = %XPmix
…What gas has the highest partial pressure in our blood
under no rmal condi t ion? ...
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Avogadro’s Law (1811,
«molecular hypothesis»):
1 mol (6,0231023 molecules) of any gas
under the same t and P occupies equal volume – 22,4 l
Molar mass (in g/mol) is numerically equal to
relative molecular mass (in Daltons):
Helium 4 Carbon Dioxide 44
Oxygen 32 Nitrous Oxide 44
Nitrogen 28 Xenon 131
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Pressure-Regulating and
Pressure Relief Valves
From: Bowie E, Huffman LM: The anesthesiamachine: essentials for understanding,
Madison, Wis, 1985, Ohmeda, a Division of BOC Health Care
P = F/S F = PS
Why does thepressure
reducing valve
freeze?
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Pressure
Measurement
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Flow
Measurement
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Flow
Measurement:
Ancient
Rotametric
Flowmeters
Dräger apparatus (ca. 1910):
Munchen, Euroanaesthesia-2007
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Flow Measurement
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Volume
Measurement
V = Q(t)dt
http://www.anesth.hama-med.ac.jp/AneDepartment/m-engstrome300.jpg
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Hagen-Poiseuille’s Law (1840)
and Reynolds’ number (1883)
R crit 1160
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Heat Capacity
and Heat ConductivitykJ/kgК W/mК
Nitrogen (N2) 1,04 0,024
Oxygen (O2) 0,91 0,024
Air (mixture) 1,01 0,024
Carbon Dioxide (CO2) 0,88 0,023
Helium (He) 5,02 0,140