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Definition
At a Constant Temperature, the volume of a given mass of gas varies inversely with the absolute pressure
V=1/P
V1P1=V2P2 |
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At constant pressure the volume of a given mass varies directly with the temperature.
V=T or V/T=k
V1/T1=V2/T2 |
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At constant Volume, the absolute pressure of a given mass varies directly with the absolute temperature
P=T
P1/T1=P2/T2 |
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Is Hypothetical
Consists of identical particles of zero volume
No intermolecular forces
Constituent atoms or molecules undergo perfectly elastic collisions with the walls of the container |
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The product of the volume of a gas and its pressure over the temperature is equal to a constant.
PV/T=k
P1V1/T1=P2V2/T2 |
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Definition
Equal volumes of gasses at the same temperature and pressure contain the same number of particles.
Avagadros law together with the combined gas law forms teh ideal gas law |
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| 6.022x10^23 particles per mole |
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8.314472 pa.m^3/mol.K
0.0821 L.atm/mol.K |
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Definition
| the total pressure exerted by a gaseous mixture is equal to the sum of the partial pressures of each individual component in a gas mixture. |
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| Temperature above which a substance cannot be liquified no matter how much pressure is exerted. |
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| occurs when the pressure of a gas is increased |
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Definition
| Occurs when the pressure of a gas is decreased |
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Term
| Joule Thompson Effect is an example of what? |
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Definition
| Adiabatic Cooling - cryoprobe |
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Definition
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Definition
| Blue 745psi 1590L (400L left when all liquid is gone) |
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Definition
| Rate of change of a quantity at any time is proportional to the quantity at that time |
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Time that it takes the quantity measured to reach 50%
t1/2=time constant x 0.693 |
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Definition
| Time it takes for the process to end assuming the first rate of change continued |
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Definition
| The ability for a given substance, the solute, to dissolve in a solvent. It is measured in terms of the maximum amount of solute dissolved in a solvent at equilibrium. The resulting solution is called a saturated solution. |
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Definition
| At a particular temperature the amount of a given gas dissolves in a given liquid is directly proportional to the partial pressure of the gas in equilibrium with the liquid. |
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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 equilibrium. |
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Definition
| Process by which the molecules of a substance transfer through a layer of area such as the surface of a solution |
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Definition
| Rate of diffusion of a substance across a unit area is proportional to the concentration gradient |
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Definition
| Diffusion rate is equal to the reciprocal of the square root of the molecular weight. |
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Definition
| osmotic pressure related to proteins |
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| Colligative Properties that are affected by osmolarity |
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Definition
Osmotic Pressure
Boiling point elevation
Freezing point depression
Vapor pressure reduction |
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| What in Anesthesia do Washout Curves apply? |
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Definition
Dye Dilution Technique
Thermodilution Technique (PA cath)
Cardiac Output L/Min
Measure Concentration of drugs in body
Nitrogen Washout Curve |
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| How Many Liters in one Mole |
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Definition
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| What the the Nitrogen Washout curve a measure of? |
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Definition
| FRC Functional residual capacity |
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| As temperature increases, do gases dissolve more or less? |
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Definition
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| What would an ideal anesthetic be like in regards to solubility, and partition coefficients? |
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Definition
Act quickly = highly insoluble in blood = low blood gas partition coefficient
Achieve anesthesia at very low concentrations = be very potent = highly soluble in fat(brain) = high oil gas partition coefficient. |
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| The amount of gas, which dissolves in a liquid, depends on 4 things: |
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Definition
The partial pressure of the gas,
The temperature of the liquid,
The nature of the gas,
The type of liquid. |
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| Equilibrium and Speed relate to what partition coefficient? |
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Definition
| Blood-Gas Partition Coefficient |
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| What is true about highly insoluble gases? |
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Definition
Equilibrates quickly
Less Potent |
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| Oxygen dissolves in blood at what partial pressure? |
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Definition
| 0.003cc/100cc/mmHg partial pressure |
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| Co2 dissolves in blood at what partial pressure? |
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Definition
| 0.067cc/100cc/mmHg partial pressure |
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Term
What are the solubility coefficients of the following at 37C
N2O
Ether
Halothane |
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Definition
N20 = 1.4
Ether = 65
Halothane = 224 |
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| If you have a diffusion with the alveolar membrane, is it more likely to show up as hypoxemia or hypercarbia? |
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Definition
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| What law is used in the measurement of Osmolarity? |
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Definition
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| Depression of vapor pressure of a solvent is proportional to the molar concentration of solute |
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Definition
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| What is an Azeotrope and give some examples |
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Definition
A mixture which vaporizes in the same proportion as its constituent volume proportions.
Alcohol 96% Water 4%
Ether 1part Halothane 2parts |
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| In terms of proportion, what is true about Ficks law? |
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Definition
| Diffusion is directly proportional to area |
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| 2 moles of a gas are dissolved in 22.4L of a liquid. what is the osmotic pressure in kPa? |
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Definition
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| What is a factor that does not effect diffusion? |
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