| Question |
Answer |
| The ability for a given substance, the solute, to dissolve in a solvent. | Solubility |
| Measured in terms of maximum amount of solute dissolved in a solvent at equilibrium. | Solubility |
| The resulting solution is called | Saturated solution |
| Gas over a liquid at a particular temp | Henry's Law |
| At at a particular temperature the amount of a given gas dissolves in a given liquid is directly proportional to other partial pressure of the gas in equilibrium with the liquid | Henry's Law |
| Particularly relevant to scuba divers
| Henry's Law |
| as you increase the pressure linearly for a gas dissolving in a liquid a proportional amount of gas will dissolve in a liquid
| Henry's Law |
| Build up saturation of nitrogen, when you resurface to quickly, it comes out of solution in the jts and tissue, this is | The Bents or The Caisson's |
| Henry's Law only applies for | constant temperatures |
| as temperature increases gases dissolve | less
|
| Pressure independent function | Ostwald solubility Coefficient |
| as the ratio of the amount of substance present in one phase compared with another, the two phase being equal volume and equilibrium | Partition Coefficients |
| Which gas is more soluble in the blood:gas coefficients?
N2O, ether, halothane
What are there bld:gas coefficients | Ether (12)
Halothane(2.3)
N20(0.47) |
| The greater the insolubility
(more equilibrium or speed) | the quicker induction rate |
| Advantage of N20 | has a quicker induction rate |
| Disadvantage of N20 | can lead to diffusion hypoxemia (reverse of 2nd gas effect)
tx: extubate with 100% o2 |
| more soluble=more potent
| oil:gas coefficient (effect) |
| less anesthetic to achieve desired clinical effect | potency |
| more insoluble=quicker induction rate | bld:gas coefficient(equilibrium or speed) |
| which gas is more potent in bld | Ether |
| which gas is more potent than ether | Halothane |
| on the log scale with gas is most potent on pg 7 | methoxytilurane |
| Oxygen dissolves in blood at | 0.003cc/100cc/mmHg partial pressure |
| C02 dissolves in blood at | 0.067cc/100cc/mmHg partial pressure |
| rate of change of a quantity of any time is proportional to the quantity at that time | exponential process |
| process by which the molecules of a substance transfer through a layer or area such as the surface of a solution | Diffusion |
| smaller molecules diffuse | faster |
| rate of diffusion of a substance across a unit area is proportional to the concentration gradient | fick's law |
| this is affected by solubility of gas diffusing into liquid medium | rate of diffusion |
| Oxygen and Carbon Dioxide rates of diffusion are different therefore more likely to become | hypoxemic |
| Do liquid or gases take longer to diffuse | liquids |
| Diffusion Rate= Reciprocal of the square root of the molecular weight | Graham's Law |
| what is Graham's law equation | 1/√MW
1 divided by the square root of MW=molecular wt |
| Diffusion equation | (p1-p2)(area)(solubility)/
(memb. thickness)(√molecular wt)
|
| what is diffusion proportional to | tension gradient (p1-p2), solubility, and directly proportional to membrane area |
| what is diffusion inversely proportional to | membrane thickness, the square root of MW of the substance diffusing |
| usually occurs with a semi permeable membrane, this membrane is semi permeable to one or more solutes. | osmosis |
| moles per liter | osmolarity |
| moles per kilogram | osmolality |
| osmotic pressure related to proteins | oncotic pressure |
| body osmolarity is | 300mmol per liter |
| difference in osmolar gradient | oncotic pressure |
| depression of vapor pressure of a solvent is proportional to the molar concentration of solute (measurement of osmolarity) | Raoult's Law |
| factors that effect osmolarity | osmotic pressure, freezing pt depression, vapor pressure reduction, and boiling pt elevation.
(colligative properties) |
| a mixture which vaporizes in the same proportion as its constituent volume proportions | Azeotropes |
| thermal state of a substance, determines whether heat will flow to or from the substance | Temperature |
| a form of energy, transfer from hotter to cooler substance, energy is in the form of kinetic energy | heat |
| SI unit of temperature | kelvins |
| determined by general metabolic rate of person | heat production |
| heat production= | 50 W/m²=80 Watts total |
| four principle routes with typical heat losses | Radiation, Convection, Evaporation, Respiration |
| what are the heat losses in percent | Radiation 40%
Convection 30%
Evaporation 20%
Respiration 10% (evaporation 8%,heating of air 2%) |
| carries away heat, cooler object absorbs the heat. occurs in OR
accounts for 50% heat loss | Radiation |
| Adjacent layer of air is heated, that heated air rises carrying away heat. | Convection |
| due to loss of latent heat of vaporization (liquid on the skin) as the liquid evaporates it sucks heat out of the body | Surface Evaporation |
| small part of heat loss, accounts for 8% of humidifying inspired air | Respiration |
| Inspiration of dry anesthetic gases may account for intra-op | hypothermia |
| physiologic control of temp is mediated by | hypothalamus |
| body temp below 35 degrees C | hypothermia |
| fever, may be due to endogenous pyrogens or from bacterial infections | Pyrexia |
| Succinylcholine and volatile anesthetics are known triggering agents for | malignant hyperthermia |
| occurs when skin at or higher than 45 degrees for prolonged time | thermal burns |
| quantity of heat required to increase the temperature of an object | Specific heat capacity |
| SI unit of specific heat capacity | J/(kg k) |
| amount of heat required to raise the temperature of a given object by 1 kelvin | heat capacity |
| SI unit of heat capacity | J/K
Joules per degree of kelvin |
| amount of heat required to raise the temperature 1 kilogram of a substance by 1 kelvin | specific heat capacity |
| 4.18 Joules = | 1 calorie |
| 4.18kJ= | 1 kilocalorie=1C |
| calculated by knowing the specific heat comtent, mass, and temperature | body heat content |
| change of state without change in temperature, requires energy | latent heat |
| joules per sec | watts |
| body generates how many watts? | 80 |
| energy used when a substance change state from a liquid to a gas | latent heat of vaporization |
| the heat required to convert 1kg of a substance from one phase to another at a given temp. | specific latent heat |
| SI unit for specific latent heat | Jkg^-1 |
| at temperature decreases the specific latent heat | increases |
| N20 critical temperature is | 36.5 |
| critical temperature for 02 | -116 C |
| ways to conserve energy use | humidified gases
circle circuit system
humidity conservation device |
| humidity in upper trachea | 34mg/L (humidify air)
9.6 watts |
| warming 02 | 2 watts |
| universal gas law | pv=nRt
R=0.0821 L atm mol-¹K-¹
p=pressure
v=vol
n=#'s moles of gas
R=gas constant
T=temp(K) |
| 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. | Dalton's law |
| SI units for pressure | pascals |
| going form one force to another set of forces is called | Van de Waals Forces |
| consists of identical particles of zero volume
hypothetical gas | ideal gases |
| equal vol of gases, at same temp. and pressure contain the same # of particles or molecules | Avogadro's Hypothesis |
| one mole of ideal gas occupies | 22.4 L @STP |
| how many liters of N20 is in a full tank | 1590 |
| the uptake of a volatile agent is increased when it is administered simultaneously with N20 | Second Gas Effect |
| One mole of particles of solute in 22.4L produces | 101.35kPa (1atm) |
| half life = | time constant * logℯ=time constant*0.693 |
| pressure= | force/area |
| force= | pressure * area |
| volume= | distance*area |
| distance= | volume/area |
| work= | pressuure*vol. |
mr. charles11
