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9 Cards in this Set
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Kinetic Molecular Theory

1.Gas molecules are dimensionless points 2.temperature is an indirect measure of molecular kinetic energy (higher temp = faster rxn) 3. Gas mlcls are in canstant, random, straighty line motion 4. Gas mlcls collide w/ each other and the container walls with no loss of energy 5. Gas mlcls exert no attractice/ repulsive force on on another


Pressure

ration of force exerted divided by the surface area over which the force is done
 force is caused by collisions  barometer and manometer * Pv= nRT 

Combined Gas Law Equation

* P1V1/n1T1 = P2V2/n2T2
Rigid container neither expands or contracts, initial and final volumes equal Closed System nothing in, nothing out, initial and final moles equal Insothermal constant temp. cancel out variables that don't change in the problems 

Boyle's Law

if you study the P and V of a gas, you get Boyle's Law: * P1V1= P2V2
(smaller volume= higher pressure) 

Charles' Law

Shows relationship between V and T of a gas
provides basis for concept of absolute zero (0= 0 volume) * V1/T1 = V2/T2 

Avogadro's Principle

When you study the volume and moles of a gas
* V1/n1 = V2/n2 

Dalton's Law of Partial Pressures

if you have a mixture of gases, then the total pressure is simply equal to the sum of each of the individual partial pressures
* Ptot= Pn add the gase pressures together if they are simply combined in a container 

Molecular Speed

gas mlcls are in constant motion, but do not travel at one constant speed
temp and molar mass effect speed Boltzmann Distribution at higher temps. the curve flattens out more and stretches *Urms = square root of 3RT/M 

Effusion and Diffusion

Effusion escape of a gas through a small hole
Diffusion spreading of one gas through another * U1/U2 =square root of m2/m1 to compare rates of diffusion or effusion 