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PHYSICS CHAP 6 Flashcards

1
Q

R constant value L atm/mol-1 K-1(most common)

A

0.082057 L atm/mol-1K-1

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2
Q

R in SI units

A

8.314 J/mol/K (relationship between temp and kinetic energy)

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3
Q

1 standard mole volume at atm

A

22.7L

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4
Q

Standard temp

A

0C or 273.17K

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5
Q

Gas density depends strongly on

A

temperature and pressure(can calculate density if temp and pressure are known)

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6
Q

Non-reacting gases are additive

A

1L air is 0.79L N and 0.21 L O2

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7
Q

Partial pressure is

A

the pressure exerted by an individual gas in a mixture

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8
Q

What is Daltons Law?

A

the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases

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9
Q

how to find partial pressure

A

.21 (gas) x 760(atm)

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10
Q

Standard atm pressure

A

760mmHg

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11
Q

If the air is gradually cooled while maintaining the moisture content constant, the _______ __________ will rise until it reaches 100%.

A

relative humidity

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12
Q

This temperature, at which the moisture content in the air will SATURATE the air, is called the ______ _______.

A

Dew Point

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13
Q

Assumes that the molecules are very small relative to the distance between molecules. The molecules are in constant, random motion and frequently collide with each other and with the walls of any container. What law is this?

A

Kinetic Theory of Gases

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14
Q

is simply the sum of the mass of the molecules divided by the volume which the gas occupies

A

Density of a gas

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15
Q

is a measure of the linear momentum of the molecules. As the gas molecules collide with the walls of a container, the molecules impart momentum to the walls, producing a force that can be measured.

A

pressure of a gas

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16
Q

is a measure of the mean kinetic energy of the gas. The molecules are in constant random motion, and there is anenergy(mass x square of the velocity) associated with that motion.

A

the temperature of a gas ( the higher the temp, the greater the motion)

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17
Q

Temp is directly proportional to the average

A

KE

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18
Q

Boltzman constant

A

is equal to the ideal gas constant R divided by AN. (treats individual molecules, while the ideal gas constant deals with moles of molecules)

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19
Q

AN is the number of molecules in a

A

mole

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20
Q

Flicks Law equation

A

DxAxPdifference/T

p1-p2)(area)(solubility)/(membrane difference)(sq rt molecular weight

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21
Q

Dissolved O2 in blood

A

0.003ml/100ml blood/mmHg

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22
Q

CO2+H2O—->

A

H2CO3(carbonic acid)

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23
Q

H2CO3+2 NaOH(Na hydroxide) + Heat————>

A

Na2CO3 + 2 H2O

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24
Q

Na2CO3 + Ca(OH)2 (ca Hydroxide)——–>

A

CaCO3(Ca carbonate) + NaOH

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25
4 Quantities that describe state of a gas
pressure, temperature, volume, and number of moles
26
Boyle's law
volume is inversely related to pressure (temp constant)
27
Charle's Law
Volume is directly proportional to the absolute temperature (pressure constant) under constant pressure
28
Avogadro's Law
Volume of a gas is directly proportional to the number of gas molecules ( temperature and pressure constant)
29
Classic example of Charle's law
Cuff on ETT or LMA
30
Example of Boyle's Law
Breathing, inspiration increases volume and decreases pressure
31
ETT cuffs are ______ volume and ______ pressure
high, low
32
Avogrado's Number
6.022x10^23
33
Gay-Lussacs Law
Pressure is directly proportional to temperature if volume is constant.
34
How to remember gas laws triangle
Can these Girls possibly Be violinists?v v
35
Ideal gas Law equation
PV=nRT
36
If the pressure on the gas isn't too ______, and the temp isn't too _________, real gases approximate ideal behavior.
high, low (ideal gases do NOT exist)
37
The warmer the air, the _______ water the air will hold.
more
38
Temperature goes down, the relative humidity goes _______.
up
39
The solubility of water in air _________ with increasing temperature.
increases
40
The average KE of a gas depends only on the _________.
temperature
41
T/F: The average KE is the same for gases at the same temperature. different gases have the same average KE if their temperatures are the same.
True, average KE depends on temp and not the identity of the gas.
42
The movement of a gas through a small opening is called
effusion(effusion and diffusion are substantially the same process)
43
the movement of a substance from an area of higher concentration to an area of lower concentration is
diffusion
44
Grahams Law states that the rate of effusion is
inversely proportional to the square root of the molecular mass
45
According to Ficks law diffusion is inversely proportional to
membrane thickness and sq root of the molecular weight
46
Describes the scenario in which the rate at which gas is transported away from functioning alveoli and into tissues is principally limited by the diffusion rate of the gas across the alveolar membrane.
Diffusion-Limited Gas Exchange
47
Describes the scenario in which the rate at which gas is transported away from functioning alveoli and into tissues is principally limited by the rate of blood flow through the pulmonary capillaries and thus across the alveolar membrane.
Perfusion-limited Gas Exchange
48
whats the law behind diffusion hypoxia?
Ficks Law
49
fick's law of diffusion for gases explains
concentration effect, second gas effect, diffusion hypoxia, and why N2O leads to increase in volume or increase in pressure in gas spaces in the body.
50
Even though CO2 is larger than O2, CO2 diffuses 20x faster across the alveolar and capillary membranes because
it is 20x more SOLUBLE
51
The process by which the fetus receives O2 and drugs is
simple-diffusion across a membrane
52
value of dissolved O2 in blood
0.003 mL/100ml blood/mmHg partial pressure of O2
53
What law permits the calculation of dissolved O2 and CO2 in blood?
Henry's law
54
The amount of gas dissolved is _______ proportional to the temperature.
inversely
55
Ostwald's solubility coefficient; the _______ the coefficient the ________ readily the gas dissolves in the liquid.
higher, more THE TWO PHASES MUST BE SPECIFIED ex blood:gas
56
The blood gas partition coefficient is also known as the
Ostwald coefficient
57
What is the Meyer Overton rule?
agents with increased oil solubility have greater potency
58
Vander Waals relationship assumes that gas molecules have _______ volumes and that gas molecules _______ one another.
finite, attract
59
What equation deal with real gases deviate at high pressure and/or low temps?
Vander Waals
60
Example of joule-thompson effect?
as a cylinder of compressed gas empties, the cylinder cools. Also how a cryoprobe works. "Joules cools"
61
The ______ in temperature of the air during adiabatic compression tends to ______ the pressure on account of the _______ in volume. What could this trigger in anesthesia machine?
increase, increase, decrease In theory the heat associated could occur when opening valves on am and trigger fire/explosion.

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