Chapter 8-The Gas Phase Flashcards
Pressure conversions 1 atm
760 MMHG
760 torr
101.325 kPa
Standard temperature and pressure
0°C and 1ATM pressure
Ideal gas definition
A hypothetical gas that has no intermolecular forces and occupies no volume.
Ideal gas law
PV=nRT
Combined gas law
(PV/T)1=(PV/T)2
Calculation of density from ideal gas law
Density= P(mm)/RT
Avogadro’s principal
1 mole of gas will occupy 22.4 L at STP
Boyles law
Ideal gas comparison constant constant temperature
Charles law
Ideal gas comparison at constant pressure
Gay-Lussac’s Law
P1/T1=P2/T2
Ideal gas comparison with constant number of moles and volume
Dalton’s law of partial pressure
In a container of mixed gases, each gas contribute to the overall pressure relative to the number of moles of that gas/the total moles of gas
Henry’s law
Defined vapor pressure, the pressure exerted by evaporated particles above the surface of a liquid.
Vapor pressure
As vapor pressure above its solution increases, the concentration of that solution will increase as gas is forced back into solution
Average molecular speed eqn
KE= 1/2mv^2 =3/2 kBT
Root mean square for speed
Sqrt((3RT)/m.m.)
Diffusion
Movement of particles from high concentration to low concentration
Graham’s law
The rates at which gases to fuse is inversely proportional to the Square root of their molar mass
Effusion
The flow of gas particles under pressure from one compartment to another through a small opening