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Kinetic Molecular Theory of Gas
 Particles are separated by large distances
 They are in random motion
 They do not form attractive or repulsion forces on one another
 Avg Kinetic Energy α absolute temp
 so T ↑, Ek↑

p = force/area
gas particles colliding with walls of the container

remember this formula
P1V1/T1 = P2V2/T2
PV = nRT

Boyle's Law
relationship b/t P and V
P1V1 = P2V2
@ constant T

Charles Law
 Volume and Temperature @ constant pressure
 V1/T1 = V2/T2
As Temp increases, Volume increases (proportional)
*Always use kelvin

C to Kelvin
K = C + 273.15

Avagadros Law
moles (n) and volume relationship
v1/n1 = v2/n2
so P1V1/n1T1 = P2V2/n2T2

Ideal Gas Equation Law
PV = nRT
R is gas constant = .08206 Latm/molar K

Standard Temp and Pressure (STP)
1 mol of gas at 0C (273.15K) + 1 atm
PVnRT (solve for V)
V = nRT/P


Dalton's Law of Partial Pressure
Gas Mixtures
 Ptotal = ΣPi
 Ptotal = Pn + Po + Par

Mole Fractions (Xi)
Tells the relative amounts of a gas mixture
 Xi = ni/ntotal
 (no units)

Consider the following regarding Mole Fractions
 1. Mole fraction of a component is < 1
 2. Sum of mole fractions for all components = 1
 3. Mole fraction is dimensionless
Xi = Pi/Ptotal

