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gas laws

Something quick to memorize all the materials

termsconcepts/equations
4 Postulates of Kinetic Theory Spherical molecules in constant, random straight-line motion “Elastic” collisions Negligible masses No interactions
Ideal Gas Gas that obeys all 4 assumptions of the kinetic theory all of the time. It doesn’t exist. It’s a model.
Real Gas Most real gases obey the kinetic theory most of the time.
Which assumptions of the kinetic theory hold up? Spherical molecules in random, straight-line motion “Elastic” collisions
Which assumptions of the kinetic theory break down? Negligible masses No interactions
When do the assumptions of the kinetic theory break down? When the gas molecules are close to each other.
When are the gas molecules close to each other? At high pressure & low temperature.
When are the gas molecules far apart from each other? At low pressure & high temperature.
How do the gas molecules act when they are far apart from each other? good
What are the properties of gases? Have mass Take the shape & volume of their container Compressible Diffuse Exert Pressure
Pressure Force/Area
Pressure results from? Collisions of the gas molecules with the walls of the container.
Pressure depends on? (microscopically) # of impacts per unit time and force of each impact
Pressure depends on? (macroscopically) # of gas molecules per unit volume And temperature
Temperature A measure of the avg. kinetic energy of the particles of a substance.
4 variables needed to completely describe a gas-phase system? Temperature Pressure Volume # of moles
Boyle's Law For a fixed mass and temperature, the pressure-volume product is a constant.
Boyle's Law PV = k where k = a constant
Boyle's Law P1V1 = P2V2
Graph of Boyle’s Law Hyperbola – it’s an inverse relationship!
Double the pressure Volume goes to ½ the original volume
Triple the pressure Volume goes to 1/3 the original volume
Halve the pressure Volume goes to 2 X the original volume
Quadruple the pressure Volume goes to 1/4 of the original volume
Which temperature scale has a direct relationship to molecular velocity? Kelvin: 0 K means 0 speed.
Math expression of Volume & Kelvin Temperature V1/T1 = V2/T2 Charles’ Law
What happens to the volume when the Kelvin temperature is doubled? The volume doubles!
What happens to the volume when the Kelvin temperature is tripled? The volume triples!
What happens to the volume when the Kelvin temperature is halved? The volume is halved!
What happens to the Kelvin temperature when the volume is halved? It’s halved!
Math expression for pressure & temperature. P1/T1 = P2/T2 Gay-Lussac’s Law
What happens to the pressure when the Kelvin temperature is doubled? The pressure is doubled.
What happens to the pressure when the Kelvin temperature is halved? The pressure is halved.
What happens to the pressure when the Kelvin temperature is tripled? The pressure is tripled.
What happens to the Kelvin temperature when the pressure is doubled? The Kelvin temperature is doubled.
What is Avogadro’s Principle? Equal volumes of gases at the same temperature & pressure have equal numbers of molecules.
What is Dalton’s Law of Partial Pressures? Ptot = P1 + P2 + P3 + P4 + …
Created by: user-1782768
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