Gases
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Kinetic molecular theory
a gas can be understood as tiny particles bouncing around in a space. the pressure on the walls of a container result in of elastic collisions.
Average kinetic energy equation
U= 3/2RT R= constant T= temperature
Brownian motion
random particle movement
Ideal gas
assumptions: - gas particles have no volume (do not take up space) - gas particles experience no attractive or repulsive forces
Ideal gas behvavior
a high temperature, large volume, and low pressure makes them more like a gas
Boyle’s Law
pressure and volume of a gas are inversely related P1V1=P2V2
Charle’s law
volume and temperature of a gas are directly related V1/T1=V2/V2
Avogadro’s law
Volume of gas is directly related to the number of moles of a gas particle V1/n1=V2/n2
At STP (273 K and 1 atm)….
1 mole of gas= 22.4 L of space this is the molar volume
Ideal gas law equation
PV=nRT R= 0.08 L atm/molK or 8.31 J/molK
Real gases
-acknowledge gas have size and there are interactions
Real gases equation (Van Der Waals equation)
(P + a/Vm^2) (Vm - b) =RT a= attractive intermolecular forces b=size of particles
Real gases under extreme pressure or low tempueratire
have a high pressure when compared to ideal gas and a low pressure when compared to an ideal gas at low temperatures
Dalton’s law
total pressure is equal to individual pressures of each gas present in the solution pgas= (xgas)(ptotal) xgas= mole fraction
Graham’s law
when a gas is diffusion, smaller and lighter particles will escape faster r1?r2=SQRT (m2/m1)