Chapter 5 Flashcards
(18 cards)
Pressure equation
P = force/area
pressure at sea level is
usually 760 mmHg
one atmosphere is defined as
760 mm Hg
Boyle’s Law
as P increases, V decreases with constant T
Charles’s Law
as T increases, V increases with constant P
aka: the hot air balloon law
Gay-Lussac’s Law
as T increases, P increases with constant V
Combined Gas Law
P1V1 P2V2
———– = ————-
T1 T2
Avogadro’s Law
equal volumes of a gas at the same T and P contain equal numbers of molecules
STP
standard temperature and pressure; pressure of 1atm and temp of 273K
What volume of gas at STP contains 1 mole of molecules?
22.4 L
Ideal gas law
PV = nRT
partial pressure
the pressure exerted by a component of an ideal gaseous mixture
dalton’s law of partial pressure
the total pressure of a gas mixture is the sum of the partial pressures of the components of the mixture
low oxygen levels cause
hypoxia
high oxygen levels cause
oxygen toxicity
effusion
the process by which a gas escapes from a container into a vacuum through a small hole. rate of effusion is inversely proportional to the square root of the molar mass of the gas
Graham’s Law
gas molecules with smaller masses diffuse (and effuse) faster than gas molecules with larger masses
diffusion
the process by which molecules spread out in response to a concentration gradient
