Molecular Thermodynamics II Flashcards
Gibbs Phase Rule
F = C - P + 2
where F = degrees of freedom, C = number of components and P = number of phases
Clapeyron Equation
dP / dT = ΔS / ΔV = ΔH / TΔV
Clausius-Clapeyron Equation
dP / dT = PΔS / RT = PΔH / RT²
Linearised Clausius-Clapeyron Plot
d ln(P) / d (1/T) = -ΔH / R
Activity
α = P / P₀
where P = pressure in solution and P₀ = pressure in the pure system
Activity Coefficient
γ = α / x
If γ > 1 the affinity is weaker
If γ < 1 the affinity is stronger
γ = 1 is ideal
Raoult’s Law for Solvent
α = x
when x is approximately = 1
Henry’s Law for Solute
α is directly proportional to x
when x «_space;1
P = kₕx
Boiling Point Elevation
ΔTb = Kb x m₂
where m₂ = solute molality and Kb is the ebullioscopic constant
Freezing Point Depression
-ΔTf = Kf x m₂
where m₂ = solute molality and Kf is the cryoscopic constant
Osmotic Pressure (van’t Hoff’s Law)
Π = RTc₂