Lecture 4 Formulas Flashcards
Boyle’s Law
At constant temperature, volume of a gas varies inversely with absolute pressure
T=PV
Derived from PV=nRT
P1V1=P2V2
Charles’ (Gay Lussac’s) Law
At constant pressure, the volume of a gas varies directly with absolute temperature
nR/P=V/T
V1/T1 = V2/T2
The Third Law
At constant volume, the absolute pressure of a gas varies directly with the absolute temperature
nR/V = P/T
P1/T1 = P2/T2
Standard Temperature and Pressure
STP
T = 273K or 0C
P = 760 mmHg
Room Temperature and Pressure
T = 293K or 20C P = 760 mmHg
Body Temperature and Pressure
310K or 37C
P = 760 mmHg
Dalton’s Law of Partial Pressures
In a mixture of gases, the pressure exerted by each gas is the same as that which it would exert if it occupied its own container.
Vx/Vy = Px/Py
Avogadro’s Hypothesis
Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. At STP - 1 mole of gas occupies 22.4L At RTP - 1 mole of gas occupies 24.0L At BTP - 1 mole of gas occupies 25.4L Avogadro's Number 6.022x10^23
E Cylinder
E cylinder tare weight is approximately 6kg
Volume = 4.5 L
Alveolar Oxygen Equation
PAO2 = FiO2 (PB-PAH2O) - (PACO2/R)
PAO2 - partial pressure of oxygen in the alveoli
FiO2 - fraction of oxygen
PB - barometric pressure
R = Respiratory quotient (carbs = 1, proteins = 0.8, fats = 0.7, average = 0.8)
PAH2O is pressure water = 47 mmHg
Alveolar Oxygen
At room air PAO2 = 100 mmHg
At 50% O2 PAO2 = 300 mmHg
At 100% O2 PAO2 = 660 mmHg
Gas vs Vapor
Gas is a substance that is above its critical temperature at room temperature (O2 and N2)
Vapor is a gas substance that is below its critical temperature. (N2O,CO2, Sevo)
Critical Temperature N2O=36.5
Critical Temperature O2 = -119C
Filling ratio
US = 0.68
UK = 0.65 or 0.75
Mass of N2O/Mass of Water to Fill Cylinder
Ideal Gas Constant
8.31 J/mol K
62 mmHg L /mol K
Water Vapor Pressure
Water at 37C is 47mmHg
6.3kPa