Gases Flashcards
How much volume does 1 mol of an ideal gas occupy?
22.4 L
What are the standard temp and pressure for an ideal gas?
273 K (0º C)and 1atm pressure
What happens when a mercury barometer is placed at the top of a mountain? At 10m under water?
At the top of the mountain where pressure is lower, the column falls. At 10m under water, where hydrostatic pressure is larger, the column rises.
What is the ideal gas law?
PV=nRT
Where R= 8.21x10^-2 Latm/molK or 8.314 J/K*mol
How can ideal gas equation be used to determine density?
p=PM/RT Where P is pressure, M is molar mass, R is constant and T is Temperture
How are pressure and volume related?
They are inversely related
P1V1=P2V2
How’s are temperature and volume related?
They are directly proportional.
V1/T1=V2/T2
How is temperature and pressure related?
P1/T1=P2/T21
What is Dalton’s law of partial pressures?
When more than one gas is in a container, each gas acts as if it is the only gas present. So the all the pressures of the individual gas adds up to the total pressure in the container
How does partial pressure affect the solubility of a gas?
The solubility of a gas will increase with increasing partial pressure of the gas
[A1]/P1=[A2]/P2
Where [A] is the concentration of the gas
What is the kinetic molecular theory of gases?
The kinetic energy of a gas particle is proportional to the absolute temperature of the gas.
The higher the temp, the faster a molecule moves. The larger the molecules the slower they move.
All gases have the same kinetic energy at the same temperature
When do real gases tend to deviate from ideal gas laws?
At high pressures and low temperatures intermolecular forces and the volume of the gas particles become significant.
What is the Van der Waals equation?
This equation accounts for the deviation of a real gas from ideal gas laws.
(P+n^a/V2)*(V-nb)=nRT
a refers to attractive forces between molecules
b refers to the size/volume of the molecules.
