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78 Cards in this Set
- Front
- Back
that which tends to change the state or motion of an object
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force
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SI unit of force
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newton (N)
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force that will accelerate one kilogram one meter per second
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one newton (1 N)
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SI unit of pressure
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pascal (Pa)
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pressure of one newton acting over one square meter
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one pascal (1 Pa)
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approximate atmospheric pressure at sea level
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1 bar
100 kPa 760 mmHg 760 Torr 14.5 psi 1 atm 1033 cm H2O |
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relationship of pressure to force
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P = f/a
where P = pressure f = force a = area |
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type of flow in which fluid has no eddies or turbulence
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laminar
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where laminar flow through a tube is fastest
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center of tube
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required to drive fluid through a tube
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pressure differential
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Hagen-Poiseuille equation
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Q = (π P d^4) / (128 η l)
where Q = flow π = 3.14... P = pressure d^4 = tube diameter raised to the 4th power η = viscosity l = tube length |
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equation which describes the effect of pressure, tube length/diameter, and viscosity on laminar flow
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Hagen-Poiseuille equation
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index which estimates the onset of turbulent flow
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Reynolds number (cutoff is 2000)
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Reynolds number equation
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Reynolds number = vρd/η
where v = linear velocity ρ = density d = tube diameter η = viscosity |
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a decrease in this fluid property decreases the tendency toward turbulent flow
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density
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in laminar flow, as this fluid property decreases, flow increases
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viscosity
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type of flow usual in lower respiratory tract
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laminar
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type of flow usual in upper respiratory tract
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turbulent
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Laplace's law for sphere
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P = 2 X T / r
where P = pressure T = surface tension r = radius |
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its presence results in surface tension increases as alveoli distend and decreases as alveoli contract
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surfactant
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fall of pressure at a constriction in a tube
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Bernoulli effect
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tube which takes advantage of Bernoulli effect to entrain gases or nebulize liquids
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Venturi tube
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tendency of stream of fluid or gas to continue to flow along a convex surface
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Coanda effect
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states that at constant temperature the volume of a given mass of gas varies inversely with the pressure
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Boyle's Law
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Boyle's Law equation
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P ∝ 1/V
where P = pressure V = volume |
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states that at constant pressure the volume of a given mass of gas varies directly with the temperature
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Charles' Law
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Charles' Law equation
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V ∝ T
where V = volume T = temperature |
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states that at constant volume the pressure of a given mass of gas varies directly with the temperature
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Third Perfect Gas Law
OR Gay Lussac's Law |
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Third Perfect Gas Law equation
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P ∝ T
where P = pressure T = temperature |
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a change in the volume and pressure of the contents of a system without exchange of heat between the system and its surroundings
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adiabatic change
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states that in a mixture of gases the pressure exerted by each gas is the same as that which it would exert if it alone occupied the container
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Dalton's Law of Partial Pressures
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states that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules
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Avogadro's hypothesis
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Avogadro's number
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6.022 X 10^23
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Universal Gas Constant equation
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PV = nRT
where P = pressure V = volume n = moles R = constant T = temperature |
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temperature above which a gas cannot be liquified however much pressure is applied
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critical temperature
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vapor pressure of a substance at its critical temperature
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critical pressure
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critical temperature at which a gas mixture may separate into its constituents
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pseudocritical temperature
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process in which the rate of change of a quantity at any time is proportional to the quantity at that time
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exponential process
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the time a process would have been complete had the initial rate of change continued
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time constant
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relationship of time constant to half-life
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half-life = time constant X 0.693
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partial pressure of a vapor in a closed container and at equilibrium with the liquid phase
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vapor pressure
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states that at a particular temperature the amount of a gas dissolved in a liquid is directly proportional to the partial pressure of the gas in equilibrium with the liquid
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Henry's Law
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the volume of a gas which dissolves in one unit volume of a liquid at the temperature concerned
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Ostwald solubility coefficient
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the ratio of the amount of substance present in one phase compared with another the two phases being of equal volume and in equilibrium
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partition coefficient
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another word for partial pressure for gases in a solution
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tension
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a substance in its gaseous phase above its critical temperature
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a gas
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a substance in its gaseous phase below its critical temperature
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a vapor
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Dalton's Law equation
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Pmixture = P1 + P2 + P3...
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fall of alveolar oxygen concentration as a result of the dilution of alveolar oxygen by excretion of nitrous oxide
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diffusion hypoxia
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increase in concentration (partial pressure) of a gas in the alveoli when a more soluble gas diffuses quickly into the bloodstream - results in increased rate of diffusion for the second gas
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second gas effect
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point at which 50% of patients cease to move in response to a stimulus
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MAC (minimum alveolar concentration)
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rate of diffusion of a substance across a surface or membrane is proportional to the concentration gradient
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Fick's Law
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states that the rate of diffusion of a gas is inversely proportional to the square root of its molecular weight
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Graham's Law
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states that depression or reduction of vapor pressure of a solvent is proportional to the molar concentration of the solute
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Raoult's Law
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a mixture which vaporizes in the same proportions as the volume concentrations of the components in solution
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azeotrope
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pathway with length greater than width
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tube
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pathway with width greater than length
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orifice
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point at which increased pressure results in turbulent flow but below which flow is laminar
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critical point
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variable orifice flowmeter
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Thorpe tube
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contributors to body pH according to Stewart
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1) partial pressure of CO2
2) strong ion difference 3) total weak acids |
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strong ions according to Stewart
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K, Na, Cl, lactate
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weak acids according to Stewart
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albumin, phosphate
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effect of decreasing the strong ion difference on body pH according to Stewart
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decreases pH
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property of He which makes it useful for decreasing resistance to flow through narrowed lower airways
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low density
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force per area of molecules in a liquid as they interface with the gas above it
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vapor pressure
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a compressed gas is any mixture or material having in a container at least one of these
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1) >104 psia @ 130F
2) >40 psia @ 70F 3) >40 psia @ 100F for any liquid flammable material |
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to determine time left on a cylinder of nitrous oxide, you must determine the volume of gas available from both...
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the liquid phase and the vapor phase
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unit of measure for osmotic activity
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osmole
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6.02 X 10^23 particles of dissolved solute that cannot diffuse through a semipermeable membrane
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1 osmole
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pressure exerted by 1 gmw of a nonionizing, nondiffusible solute in 22.4L of water
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1 atm
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pressure exerted by 1gmw of a monovalent, ionizing, nondiffusible solute in 22.4L of water
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2 atm
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states that even in isolation from the environment, a gas cools when expanded and warms when compressed
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Poisson adiabatic equation
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Which of the following does NOT affect rate of laminar flow? pressure gradient, fluid viscosity, tube length, fluid density, tube diameter
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fluid density
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At low rates of flow, the orifice of a variable orifice flowmeter is more like what?
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a tube
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tendency toward turbulence increases when this fluid property is increased
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density
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tendency toward turbulence decreases when this fluid property is increased
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viscosity
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As tube diameter is doubled, rate of flow _________ by a factor of _____.
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increases, 16
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As tube length is halved, rate of flow ____________ by a factor of _____.
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increases, 2
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