All Sections
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
|
|
||||
|---|---|---|---|---|---|
| Solubility
🗑
|
|||||
| Solubility
🗑
|
|||||
| The resulting solution is called |
🗑
|
||||
| Gas over a liquid at a particular temp |
🗑
|
||||
| a given gas dissolves in a given pressure of the gas in equilibrium with the liquid |
🗑
|
||||
|
🗑
|
|||||
| as you increase the pressure linearly for a | 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.
🗑
|
Review the information in the table. When you are ready to quiz yourself you can hide individual columns or the entire table. Then you can click on the empty cells to reveal the answer. Try to recall what will be displayed before clicking the empty cell.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
Created by:
melbacs
Popular Chemistry sets