Chapter 5- Gas Flashcards
(16 cards)
Parameters affecting gas
Pressure
Volume
Temp
Number of moles
Properties of gas
1 volume changes with temp and pressure
2 expand to uniformly fill container
3 have no definite volume or shape
4 mix completely with any other gas in any proportions (miscible)
5 much lower density than solids & liquids (g/L)
Gas pressure
Pressure=force per area Collisions with surfaces create pressure. More particles = higher pressure More frequent = higher pressure Less area = higher pressure
Measurement of pressure
Standard atmospheric pressure
The mercury barometer
Elevation and atmospheric pressure(atm)
Atmospheric pressure decreases with altitude due to decreased density of gas molecules
Boyle’s law
The volume of gas is inversely proportional to applied pressure
T and n are fixed
P1V1=P2V2
Charles’s law
The volume of gas is directly proportional to kelvin temperature and extrapolates to zero at zero kelvin
P and n fixed
V1/t1= V2/T2
Avogadro’s law
The volume of a gas is directly proportional to the number of moles of has (at low pressures)
P and t fixed
V1/n1 = V2/n2
Amonton’s law
Gas pressure is directly proportional to kelvin temp
N and v fixed
P1/T1= P2/T2
Genera gas equation
Combining gas laws
P1V1/n1T1 = P2V2/n2T2
Ideal gas law
PV=nRT
P= pressure in ATM V= vol in liters N= moles R= 0.08206 T= temp in K
Standard temperature and pressure STP
P= 1atm T = 273k N= 1 R =22.41L Ideal gas
Gas density
D= PM/RT
Dalton’s law of particle pressure
Partial pressure = pressure contribution of a gas within a mixture
Pa= NaRT/V total
Collecting a gas over water
Ptotal=Pgas-Ph2o
Mole fraction
Na = Pa/Ptotal