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Intro to Respiratory Therapy > Chapter 54: Physical Principles > Flashcards

Chapter 54: Physical Principles Flashcards

1
Q

May be a pure element, in which atoms are the same, or a compound of different atoms

A

Molecule

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2
Q

Explains that there are three states of matter

A

Molecular theory

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3
Q

State of matter with a condensed structure in which strong intermolecular bonds determine a definite shape and volume

A

Solid

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4
Q

State of matter composed of molecules that move freely, have no definite volume, and are without definite shape

A

Liquid

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5
Q

State of matter that is compressible and completely fills an enclosed space

A

Gas

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6
Q

State of matter with strong intermolecular bonds

A

Solid

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7
Q

State of matter that is dense than gases and are fluid

A

Liquid

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8
Q

State of matter with weak intermolecular bonds and are fluid

A

Gas

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9
Q

A hot ionized gas consisting of approximately equal numbers of positively charged ions and negatively charged electrons. Often considered a fourth state of matter

A

Plasma (ex. sun, lightning)

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10
Q

Units of measurement

A

Lenth - Meter - m
Mass - Kilogram - kg
Time - Second - s
Temperature - Kelvin - k
Force - Newton - N
Pressure - Pascal - Pa
Work - Joule - J
Frequency - Hertz - Hz

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11
Q

Common unit of measurement for pressure for gases

A

cm H2O

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12
Q

Common unit of measurement for pressure for liquids

A

mm Hg

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13
Q

A dot over a symbol represents

A

The rate of change (distance over time or velocity)

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14
Q

The amount of a substance, determined by the number and type of molecules

A

Mass

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15
Q

The measurement of the pull of gravity on an object

A

Weight

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16
Q

Measured on a scale

A

Weight

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17
Q

Measured by using a balance comparing a known amount of matter to an unknown amount of matter

A

Mass

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18
Q

A mechanical energy applied to the body. The product of mass times acceleration

A

Force (F = m x a)

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19
Q

Describes the force due to to the acceleration of gravity acting on a mass. Mass times gravity

A

Weight (W = m x g)

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20
Q

A force applied to an area

A

Stress

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21
Q

Force applied at an angle

A

Shear stress

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22
Q

(Force per area) is the same concept applied to fluids, including gases.

A

Pressure (P = F / A)

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23
Q

Pressure generated by the weight of atmospheric gas above the barometer at any altitude. Drops when there is an increase in elevation

A

Atmospheric Pressure

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24
Q

The physical deformation of a structure, usually caused by stress

A

Strain

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25
The reversible deformability that can be generated by stress, yet, it returns to its original form
Elasticity
26
State of matter that is highly elastic and can be compressed relatively easily
Gas
27
State of matter that is less elastic and behaves as if it is incompressible
Liquid
28
The resistance to movement between adjacent fluid molecules
Viscosity
29
State of matter that lacks elasticity
Solid
30
Term for when the weight of a fluid generates static fluid pressure due to the force gravity
Hydrostatic Pressure
31
Fluid exits capillary since capillary hydrostatic pressure is greater than blood colloidal osmotic pressure
Filtration
32
No movement of fluid since capillary hydrostatic pressure is the same as the blood colloidal osmotic pressure
No net movement
33
Fluid re-enters capillary since capillary hydrostatic pressure is less than blood colloidal osmotic pressure
Reabsorption
34
Hydrostatic Pressure equation
P = h x p x g P = Pressure h = height p = density g = acceleration of gravity
35
Volume change caused by pressure change/stiffness of sphere
Compliance
36
Reciprocal of compliance. Returns to its original shape
Elastance
37
Law stating that at equilibrium, pressure is constant throughout the fluid, if the pressure caused by the weight of the fluid is neglected. Ignores hydrostatic pressure
Pascal's Law
38
Law that describes the tension of the wall of a sphere or cylinder. Wall tension increases with radius. A smaller structure generates a greater inward pressure, resulting in a tendency to collapse due to surface tension
Laplace's Law T = (P x r) / 2 P = (2 x T) / r T = Tension P = Pressure r = Radius
39
The tension of the surface film of a liquid caused by the attraction of the particles in the surface layer by the bulk of the liquid, which tends to minimize surface area.
Surface Tension
40
The amount of heat, or thermal energy, present in a system.
Temperature
40
Reduces surface tension. Reduces the pressure required to expand an alveolus. Also reduces the pressure differences between alveoli of different diameters
Surfactant
41
Temperature Scales
Absolute Zero: F = -460 C = -273 K = 0 Oxygen Boils: F = -297 C = -183 K = 90 Water Freezes: F = 32 C = 0 K = 273 Normal Body Temp: F = 98.6 C = 0 K = 310 Water Boils: F = 212 C = 100 K = 373
42
Fahrenheit to Celsius Conversion
C = (Fahrenheit degrees - 32) x 5/9
43
Celsius to Fahrenheit Conversion
F = 32 + (Celsius degrees x 9/5)
44
Changes in the thermal state of a system by adding or removing energy, such as when changes in pressure, volume, or temperature alter the state of a substance
Thermodynamics
45
A change of state which requires the addition of energy (heat)
Endothermic
46
A change of state which requires the release of energy
Exothermic
47
Exothermic change from gas to a liquid or solid
Condensation
48
Exothermic change from liquid to a solid
Freezing
49
Endothermic change from a solid to a gas
Sublimation
50
Endothermic change from a solid to a liquid
Melting
51
Endothermic change from a liquid to a gas
Evaporation
52
Defines the relationship between pressure, volume, temperature and the number of molecules of a gas. Pressure and volume are inversely related, whereas temperature is directly proportional to volume or pressure
Ideal Gas Law (P1 x V1) / T1 = (P2 x V2) / T2 P = Pressure V = Volume T = Absolute Temperature PV = nRT P = Pressure V = Volume n = Number of Moles R = Gas Constant T = Absolute Temperature
53
Law stating that volumes of gases combine chemically in volumetric proportions that are small whole numbers
Gary-Lussac's Law of Combining Volumes V = k x n V1 / n1 = V2 / n2 V = Volume k = Constant n = Number of Moles
54
Law states that pressure is inversely proportional to volume. If the volume of a gas is halved, pressure will double, given a constant mass and temperature
Boyle's Law P x V = k P1 x V1 = P2 x V2 P = Pressure V = Volume k = Constant
55
Law that predicts the effect of temperature on a fixed amount of dry gas. As the temperature increases, the volume increases because the faster molecules collide harder and push each other farther apart.
Charles's Law V = k x T V1 / T1 = V2 / T2 V = Volume k = Constant T = Absolute Temperature
56
Law that describes the direct relationship between pressure and temperature given a fixed mass and volume of gas
Gary-Lussac's Law of Pressure and Temperature P = k x T P1 / T1 = P2 / T2 P = Pressure k = Constant T = Absolute Temperature
57
Law that describes the behavior of physical mixture of gases and vapors
Dalton's Law of Partial Pressures Pressure of Oxygen at 1 Atmosphere PIO2 = FIO2 x Patm PIO2 = 0.21 x 760 mm Hg = 160 mm Hg PIO2 = Partial Pressure of inspired oxygen FIO2 = Fraction of Oxygen in inspired gas Patm = Atmospheric Pressure
58
Composition of Dry Air
Nitrogen = 78.08 % Oxygen = 20.95 % Carbon Dioxide = 0.03 % Argon = 0.93 % Trace Gases = 0.01 %
59
Calculation of Absolute Humidity
(16.42 - 0.73 x T) + 0.04 x T2 T = Temperature (Celsius)
60
Calculation of Relative Humidity
(Absolute Humidity / Humidity Capacity) x 100%
61
Calculation of Humidity Deficit
Content - Capacity at 37 degrees Celsius = Content - 43.8 mg/L
62
Calculation of Body Humidity
(Content/Capacity) x 100% = (Content/43.8 mg/L) x 100
63
The measurement of the actual amount of water vapor in the air or the mass of water present in a volume of gas, usually measured in milligrams per liter. Can be measured by weighing the water vapor extracted from air using a drying agent, or using meteorological equipment
Absolute Humidity

Intro to Respiratory Therapy (5 decks)

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