Essential physics for anaesthesia Flashcards
Define a gas
Define a vapor
Gas
A gas is a compressible fluid phase in which no liquid can be formed at that temperature. The threshold above which a substance exists as a gas is its critical temperature.
Vapor
A vapor is a gaseous phase which is in a state of equilibrium with the same substance in a liquid form. A vapor can exist only below its critical temperature
At what pressure does the 20ºC isotherm for N2O go from containing Vapour + Liquid to just liquid?
At what pressure does the 36.5ºC isotherm for N2O go from vapor to liquid
20ºC isotherm for N2O go from containing Vapour + Liquid to just liquid: 52 bar (52 x 100 kPa)
36.5ºC isotherm for N2O go from vapor to liquid: 73 bar (73 x 100 kPa)
Describe the names and history of the three ideal gas laws
Boyle’s law - 1662: relating pressure and volume
Charles’s law - 1787: relating volume and temperature
Gay-Lussac’s law - 1808: relating temperature and pressure
Amalgamated to form the Combined Gas Law
Define the 1st ideal gas law (Boyle’s law)
Boyle’s law states that at in a closed system at constant temperature the pressure of a fixed mass of gas is inversely proportional to the volume.
P ~ 1/V
PV = K1
Define the 2nd gas law (Charles’s law)
Charles’s law states that in a closed system at constant pressure the volume of a fixed mass of gas varies in proportion to the absolute temperature.
V ~ T
V/T = K2
Define the 3rd gas law (Gay-Lussac’s law)
Gay-Lussac’s law states that in a closed system at constant volume the pressure of a fixed mass of gas varies proportionally to the absolute temperature.
P~T
P/T = K3
What is the difference between the Combined Gas Law and the Ideal Gas Law
PV/T = k (Combined gas law)
PV = nRT (Incorporates the number of molecules present and the universal gas constant R)
Why is the pressure a gauge an accurate representation of quantity in an oxygen cylinder but not for a N2O cylinder?
O2 cylinder - O2 is above its critical temperature - therefore with a constant temperature and pressure, according to the ideal gas law P is proportional to the number of moles present (V, T, R all constant).
N2O cylinder - N20 has a critical temperature of 36.5ºC. It is therefore below its critical temperature. As the pressure increases more vapour will be condensed into the liquid phase –> N2O therefore does not conform to the ideal gas law and the cylinder must be weighed to measure its contents.
Define Dalton’s law
John Dalton observed that the total pressure is the sum of the pressures of the individual gases, as if they were alone in the same volume.
The pressure exerted by each gas is termed its partial pressure (assumed T is constant and that the gases do not react with each other)
Ptotal = P1 + P2 + P3
From this, you can derive that the fraction of the total pressure exerted by a gas in a mixture is directly proportional to its fractional composition within the mixture
e.g. Air contains 21 % of O2 by volume. Its partial pressure = 0.21 x 101 kPa = 21 kPa
Define saturated vapor pressure
As liquid continues to evaporate into a space above it, the pressure of its vapour increases. When a point of equilibrium is reached between the rate of evaporation and the rate of condensation, this vapour pressure is known as the saturated vapour pressure.
What single variable changes the SVP of a substance?
The SVP increases progressively with a rise in temperature.
What happens when the SVP equals the atmospheric pressure?
The liquid boils. The temperature at which the saturated vapour pressure equals the atmospheric pressure is the boiling point.
Define Henry’s law
At a constant temperature, more molecules are dissolved at higher pressure.
The amount of gas dissolved in a liquid is directly proportional to the partial pressure of the gas in equilibrium with the liquid.
Gas molecules dissolved inside the solution reach equilibrium when the partial pressure of the gas in solution equals the partial pressure of the gas above.
How does Henry’s law apply to volatile anaesthetic agents?
If the partial pressure of a volatile anaesthetic agent in the alveoli is doubled, once equilibrated the partial pressure and quantity dissolved in the blood will also double
How does the quantity of gas dissolved in a liquid vary with different types of gases?
For different substances, the quantity of gas dissolving in a liquid at a given partial pressure can vary hugely and is related to their solubility coefficients.
What is a partition co-efficient?
This describes the relative concentration in each of two defined phases when an agent has distributed between them at equilibrium. E.g. Blood:Gas co-efficient
How does temperature effect solubility
As the temperature increases, the molecules in the solution have more energy to get out of the liquid and so solubility falls
Conversely, a fall in temperature increases the solubility of a gas in a liquid.
What are the important differences between AC and DC current in terms of electrical safety
AC is more efficient for transmission than DC but AC is more hazardous to the body in the event of an electrocution.