Gas Laws :( Flashcards
What is the molecular theory of matter?
matter is made of molecules that can exist in solid, liquid, gas
What is the kinetic theory of matter?
molecules are in constant (random) motion and have attraction between them (van der waals forces)
What is Avagrado’s hypothesis and number?
-2 diff containers containing 2 diff gas at same temp and pressure = same number of molecules
1 mole = 6.02 x10^23 molecules
How do you determine a mole?
1 mole = 1 gm x molecular weight
i.e. 1 mole of O2 = 32 g
How many liters does 1 mole of ANY substance occupy?
How many molecules would 1 mole of O2 have and how many liters would it occupy?
(Avagadro)
22.4 liters
therefore 6.02 x 10^23 molecules of O2 = 32 g and occupies 22.4 l
How are vaporizers calibrated?
using Avagadro’s hypothesis:
-i.e. Sevoflurane = 200 g
1 mole of sevo is 200 g and occupies 22.4 l at S.T.P (standard temperature and pressure)
-so if only putting 20 g of sevo into vaporizer then = 0.1 mole, it will occupy 2.24 l when it all vaporizes
What is Boyle’s gas law?
as pressure increases, volume decreases
(when temp is constant)
V = 1/P
What is an example of Boyle’s law in anesthesia?
- reservoir bag
- E cylinder
- spontaneous breathing
- bellows
- applying pressure (squeezing) reservoir bag decreases volume
- a full E cylinder of O2 = 625 L (small volume is at high pressure of 2000 PSI), as you open tank, pressure decreases and volume increases
- (inspiration) when intrapulmonary (lungs) pressure becomes more negative (decreases), intrapulmonary volume increases
- as pressure increases, volume within bellows decreases
What is Charles’ gas law?
as temperature increases, volume increases
V/T = constant (when pressure is constant)
What is Gay-Lussac’s gas law?
as temperature increases, pressure increases (when volume is constant)
P/T = constant
What is an example of Gay-lussac’s law regarding a gas cylinder?
full cylinder of gas moves from air conditioned hospital (70 degrees F) to loading dock (100 degrees F), pressure will increase
What is the universal gas law?
PV = nRT
n = # of moles of gas (Avagadro) R = universal gas constant T = absolute temp P = pressure V = volume
What is an example of the universal (ideal) gas law regarding cylinders?
PV = nRT
-as cylinder of compressed gas empties, pressure falls
-cylinder has a constant volume
-# of moles (n) decreases as gas exits cylinder = pressure decreases
(P = n)
What is Dalton’s law?
-total pressure of gas mixture = sum of partial pressure of each gas
total P = P1 + P2 + P3
-in mixture of gas, pressure of each gas is same as if it were alone in the container
What is an example of Dalton’s law regarding the gas mixture of air?
O2 = 21% > 760 mmHg x .21 = 160 mmHg N = 79% > 760 mmHg x .79 = 600 mmHg
Determine the partial pressures of each for a mixture of inhalation anesthetic: 50% N2O 44% O2 6% Desflurane total = 100% to patient
N2O > 760 x .50 = 380 mmHg
O2 > 760 x .44 = 334 mmHg
Desflurane > 760 x .06 = 46 mmHg
What is Fick’s Law of Diffusion?
rate of diffusion across membrane is directly proportional to:
1. concentration gradient (pp diff of gas)
2. surface area of membrane
3. solubility
and indirectly proportional to
4. thickness of membrane
5. molecular weight
V (gas) = SA x solubility x pp diff/ mol wt x distance
How does Fick’s law apply to anesthetic gases?
- N2O as a second gas
- N2O concentration
- alveolar-capillary membrane
- air pockets
- ETT cuff
- placental transfer
- 2nd gas effect - high concentration of first gas (N2O) accelerates uptake of 2nd gas
- concentration effect - uptake of high volumes of N2O concentrates remaining 2nd gas
- diffusion of gas across alveolar-capillary membrane (diffusion hypoxia - gradient that is driven by hypoxia = high to low)
- expansion of air pockets - with N2O (34x more soluble than N in blood) - N2O diffusing in is > N going out
- expansion of ETT cuff with N2O use
- placental transfer of drugs and O2
What is Graham’s law?
as molecular weight increases, rate of diffusion decreases
What is Henry’s law?
increased amount of gas dissolved = increased partial pressure
How do you apply Henry’s law to ABGs if
PaO2 = 600 mmHg and PaCO2 = 35 mmHg
1. Henry's law allows calculation of O2 and CO2 dissolved in blood O2 constant = 0.003 ml/100ml/mmHg pp CO2 constant = 0.067 ml/100ml/mmHg pp PaO2 = 600 x 0.003 = 1.8 ml/100ml blood PaCO2 = 35 x 0.0067 = 0.23/100 ml blood
How do you apply Henry’s law to PaO2 when delivering O2?
- Multiply FiO2 x 5 (because 21% = 1/5 of 100%)
- if 21% RA > 21x5 = 105 mmHg x 0.003 = .315 ml/100 ml blood
- if deliver 40% FiO2 > 40 x 5 = 200 mmHg x 0.003 = 0.6ml/100 ml blood