Chapter 10 - Gases Flashcards
Boyle’s law
Volume is inversely proportional to pressure
What does kinetic molecular theory explain?
Gas behavior on molecular level:
1) molecules in continuous, random motion
2) use volume of container
3) attractive and negative forces between molecules are negligible
4) transfer of energy but average kinetic energy stays the same
5) average kinetic energy is proportional to absolute temperature
Charles’s law
Volume is directly proportion to absolute temperature
Avogadros law
Volume is directly proportional to number of moles at constant temp and pressure
Dalton’s law of partial pressure
Total pressure is equal to all partial pressures added up
Van der waals equation
N2*a/v2 accounts got attractive and repulsive forces
Nb accounts for volume of molecules
Volume increases pressure
Attractive forces decreases pressure
Graham’s law
A lighter gas has a higher effusion rate
Rate1/rate2 = sqrt (m2/m1)
Low mean free path
Frequent collisions and low average distance
High mean free path
Infrequent collisions and long distance
STP
Standard temperature pressure
0celcius 273K
22.4 L/mol
Column problem
Density of unknown
Rms speed molar mass is in
Kg/mol
Pressure rises as the temperature increases.. Two reasons why
Force molecules hitting the walls increase
Frequency of collisions with wall increases
Characteristics of a gas
Low molar mass Expand to fill container Highly compressible Low densities Molecules far apart
Manometer
Used to measure difference in pressure between atmosphere and hat of a gas in a vessel
Pgas = Patm + Pheight
