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# OAT - Chem

### Chapter 7- The Gas Phase

TermDefinition
The phases/states solid, liquid, gas
Gases molecules move rapidly, are far apart, can expand to fill any volume, take the shape of a container, and are compressible
What variables help define gases P, V, T, n
(STP) P (pressure) 1 atm = 760 torr = 760 mm Hg
V (volume) mL or L
(STP) T (temperature) 273 K
STP standard temp and pressure = 1 atm and 273K; V = 22.4L, n = 1mole
Standard Conditions 298K, enthalpy, entropy, Gibbs, voltage
Ideal Gases a hypothetical gas whose molecules have no intermolecular forces and occupy no volume; high temp, low P
Boyle's Law Under isothermal conditions, P1V1 = P2V2
Charles' Law under constant pressure conditions, V1/T1 = V2/T2
n number of moles
Avogadro's Principle when pressure and temp are constant, n1/V1 = n2/V2
Ideal Gas Law PV = nRT
R gas constant; = 8.21E-2; 8.314J/Kmol
Density mass/volume; g/L for gases
Deviations Due to Pressure as P increases, gas condenses into liquid state
Deviations Due to Temp As T decreases, gas condenses into liquid state
Dalton's Law of Partial Pressures the total pressure of a gaseous mixture is equal to the sum of the partial pressures of the individual components; Ptot= P1 + P2 + etc
P1 = Ptot (X1) Partial pressure equation
KE equation for gases avg KE is proportional to absolute T; KE = 3/2 KT
Graham's Law of Diffusion and Effusion Eq r1/r2 = [MM2/MM1]^1/2
Created by: JaeBae4444