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Principles 1 > Physics Review > Flashcards

Physics Review Flashcards

1
Q

3 physical states of a substance

A

solid, liquid, gas

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2
Q

Solid

A
  • Atoms/molecules are closely approximated due to lattice.
  • Have volume and shape
  • Motion is limited, only vibrate in position
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3
Q

Liquid

A
  • Molecules exert weaker force on each other called Van der waal forces
  • allows fluid flow, sliding, and the molecules can move throughout the substance.
  • Takes shape of container, has volume.
  • Have more kinetic energy
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4
Q

Gas

A
  • Molecules are independent of each other
  • Molecules are constantly moving
  • No definite shape or volume
  • Measured by flowmeters or respirometers
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5
Q

Inverse Relationship

A

The value of one parameter decreases as the value of the other parameter increases

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6
Q

Direct Relationship

A

Where two variables do the same thing

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7
Q

Saturated Vapor Pressure

A

Pressure exerted by a vapor when, at any one temp, an equilibrium is reached at which the same number of molecules are vaporizing as are returning to liquid

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8
Q

Boiling Point

A

The temp at which vapor pressure becomes equal to atmospheric pressure and at which all liquid changes to gas

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9
Q

Vapor pressure and boiling points are ___ related

A

inversely related

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10
Q

Force

A

That which changes or tends to change the state of rest or motion of an object
__=mass x acceleration (Newton’s 2nd law)

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11
Q

Pressure

A
  • Force applied over a surface
  • Pa = pascal
  • kPa is usual unit utilized
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12
Q

Absolute Pressure

A

gauge pressure + atmospheric pressure

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13
Q

Boyles Law

A
  • At a constant temperature, the volume of a given gas varies inversely with the absolute pressure.
  • P1 x V1 = P2 x V2
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14
Q

Charles Law

A

at a constant pressure the volume of a given gas varies directly with the absolute temperature
-V1/T1 = V2/T2

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15
Q

Gay Lussac’s Law

A

at a constant volume the absolute pressure of a given mass of gas varies directly with the absolute temperature
- P1/T1 = P2/T2

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16
Q

Dalton’s Law of Partial Pressures

A

In a mixture of gases, the pressure exerted by each gas is the same as that it would exert if it was alone in the container.

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17
Q

Avogadro’s Hypothesis

A

equal volumes of gases at the same temperature and pressure contain equal numbers of molecules (a mole)

1 mole = 6.022x10^23

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18
Q

Universal gas constant

A

Constants: PV, V/T, P/T

PV/T = universal gas constant

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19
Q

universal gas law (ideal gas law)

A

PV=nRT

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20
Q

Critical Temperature

A

the temp above which no amount of pressure can liquefy a gas

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21
Q

Critical pressure

A

the pressure to liquefy a gas at its critical temperature

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22
Q

Solubility

A

solution is a homogenous mixture of a solute (gas) in a solvent (liquid)
depends on: partial pressure of gas, temperature, gas, liquid

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23
Q

Henry’s law

A

at a certain temp, the amount of a given gas dissolved in a given liquid is directly proportional to the partial pressure of the gas in equilibrium with the liquid

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24
Q

La Chatelier’s Principle

A

a change in any of the factors in determining an equilibrium causes the system to adjust or reduce or counteract the effect of the change.

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25
Q

solubility coefficient

A

the volume of gas which dissolves in one unit volume of the liquid at the temp concerned

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26
Q

partition coefficient

A

the ratio of the amount of substance preset in one phase compared with another (the two phases being of equal volume and in equilibrium)

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27
Q

Blood gas partition coefficient

A

reflects the proportion of the anesthetic that will be absorbed in the blood verses the amount of anesthetic that will leave the blood to diffuse into tissues

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28
Q

oil gas partition coefficient

A

ratio of a gas present in oil verses in the gas state.

Indicates how efficiently a gas can access and affect the sites of action.

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29
Q

diffusion

A

the continual movement of molecules among each other in liquids or in gases. Occurs from areas of high concentration to areas of low concentration.

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30
Q

What are things that make a difference to rate of diffusion?

A
  • thickness of membrane (d)
  • size of a molecule (MW)
  • surface area of the membrane (A)
  • solubility of the gas (S)
  • pressure gradient (P1-P2 or change in P)
31
Q

Fick’s Law

A

the rate of diffusion of a substance across unit area is proportional to the concentration gradient

32
Q

Graham’s law

A

the rate of diffusion of a gas is inversely proportional to the square root of its molecular weight

33
Q

cohesion

A

internal attractive forces between like molecules trying to stick together in the smallest shape possible.

34
Q

adhesion

A

attractive forces between unlike molecules trying to stick to something different

35
Q

surface tension

A

cohesive forces at the surface of a liquid that tend to keep liquid in the most compact form.
-heating lowers ___

36
Q

P=hdw

A

pressure in liquids

37
Q

Density of H2O = 1gm/cc

Density of Hg = 13.6 gm/cc

A

convert cm h20 to mmHg: 0.74 x __

convert mmHg to h20: 1.36 x ___

38
Q

flow

A

the quantity of fluid passing a point in a given time.

F=Q/T

39
Q

laminar flow

A

fluid movement in smooth layers with no turbulence or eddies.
flow is greatest in center, becomes slower as it gets closer to a wall.

40
Q

turbulent flow

A

flow is not smooth but has swirls and eddies

41
Q

what changes resistance to flow

A
  • diameter of channel
  • length of channel
  • nature of the flow (laminar vs turbulent)
  • viscosity of fluid
42
Q

viscosity

A

frictional forces between layers within a fluid

43
Q

hagen-poiseuille equation derivative

A

Resistance = 8nL/πr4

-radius matters the most

44
Q

Poiseuille’s law

A

P1 – P2 = Resistance x Flow

looks at flow rate in relation to resistance and the pressure gradient if you have an ideal fluid and no turbulence

45
Q

Bernoulli Effect

A

Given a channel with a narrowing which then
increases, the pressure measured along the
channel is lowest at the narrowest point, often
below atmospheric
Narrowing causes increased velocity, thus
increased kinetic energy. To maintain unchanged
sum of energy, the potential energy must decrease.

46
Q

Laplace’s Law

A

Relationship of wall tension, pressure, and radius of

cylinders (vessels) and spheres (ventricles and alveoli*)

47
Q

Heat

A

kinetic energy of molecules of substance

48
Q

Calorie (cal)

A

energy to increase temp of one gram of H2O 1 degrees celcius

1kcal=C=4184 joules=energy to increase temp of 1kg H2O 1 degrees celcius

49
Q

Temperature

A

the parameter used to describe the amount of heat possessed

50
Q

F to C

A

Tc = 5/9 (Tf – 32)

51
Q

C to F

A

Tf = 9/5 Tc + 32

52
Q

C to K

A

Tk = T c + 273

53
Q

Kelvin and triple point

A
  • necessary for calculations in gas laws
  • all atomic motion ceases at 0 kelvin
  • the temperature at which water, ice, and water vapor are all in equilibrium
54
Q

First law of thermodynamics

A

heat is a form of energy and can be converted to other forms of energy, but neither created nor destroyed

55
Q

second law of thermodynamics

A

heat always flows from warmer to cooler (think high to low). There must exist a difference in temp and the two things must be in contact.

56
Q

Methods of heat transfer

A

conduction
radiation
convection
evaporation

57
Q

conduction

A

heat movement through a substance by the transfer of kinetic energy from molecule to molecule.

2% heat loss

58
Q

Radiation

A

heat transferred from warmer to cooler objects by emission and absorption of energy radiated in varying wavelengths
objects do not have to be touching
40% heat loss

59
Q

convection

A

heat transfer occurs by moving fluid (liquid or gas)

air adjacent to body is warmed, it expands and moves away, and it carries the heat away

60
Q

evaporation

A

the loss of latent heat of vaporization of moisture on the skin’s surface

latent heat of evaporation - the heat required to change liquid into vapor

61
Q

specific heat capacity

A

the amount of heat required to raise the temp of 1 kg of a substance by 1 kelvin

  • Water is standard: 1 cal/g/C = 1 kcal/kg/ C
  • 1 cal=4.18 joules
62
Q

heat capactity

A

the amount of heat required to raise the temp of an object by 1 kelvin

-calculated by multiplying the mass of the object with the specific heat capacity

63
Q

specific latent heat

A

energy required to convert 1 kg of a substance from one phase to another at a given temp (J/kg)

64
Q

latent heat of fusion

A

the heat required to change a solid to a liquid

65
Q

latent heat of vaporization

A

heat required to change a substance from a liquid to a gas at a constant temp

66
Q

latent heat of vaporization

A

heat required to change a substance from a liquid to a gas at a constant temp

67
Q

Joule-thompson effect

A

(joule is cool)
when nitrous cylinder is allowed to empty rapidly, the cylinder becomes very cold and the water vapor from the surrounding air freezes on the cylinder

68
Q

radiation (xray vs LASER) atomic structure

A

protons (+)
neutrons (neutral)
electrons (-)

69
Q

Types of electromagnetic radiation: Ionizing

A
  • releases energy by removing electrons from atoms in tissue creating atoms that are very hazardous
  • xrays, gamma rays, radiation tx for cancer, dangerous if absorbed
70
Q

Nonionizing electromagnetic radiation

A
  • discharges its energy without creating ions or removing electrons from atoms in tissues
  • infrared radiation, visible light, UV radiation, LASER
71
Q

protection from ionizing radiation

A

-DISTANCE is best form. At least 3 feet away.
-minimize TIME
-use barriers to SHEILD (lead aprons)
6 ft of air is the equivalent to 9 in of concrete or 2.5 mm lead

72
Q

Maximum yearly occupational exposure of ionized radiation

A
  • no more than 5 rem or 5000mrem
  • one CXR is 25 mrem
  • flouroscopy procedure could produce >8000 mrem
  • max exposure pregnancy is <500 mrem
73
Q

protection against nonionizing radiation

A
  • eyewear
  • nonreflective instruments
  • distance does NOT help
  • cover patients eyes with moistened gauze and exposed skin with wet towels
  • decrease % of O2 used to 30%, no use of nitrous
  • filter mask to prevent intake of the plume (cellular debris)

Principles 1 (12 decks)

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