Physical Chemistry
Formulas

Thermochemistry

ΔH = H_products - H_reactants
q = mcΔT
ΔH = ΣΔH_f(products) - ΣΔH_f(reactants)
ΔH = Σ bond energy(reactants) - Σ bond energy(products)

ΔH_total = ΣΔH_steps
ΔH is independent of path
Only depends on initial and final states

Entropy & Gibbs Free Energy

ΔS = S_products - S_reactants
ΔS > 0: increase in disorder
ΔS < 0: decrease in disorder

ΔG = ΔH - TΔS
ΔG < 0: spontaneous
ΔG = 0: equilibrium
ΔG > 0: non-spontaneous
ΔG° = -RT ln(K)

Kinetics

Rate = k[A]^m[B]^n
Zero order: [A] = [A]₀ - kt
First order: ln[A] = ln[A]₀ - kt
Second order: 1/[A] = 1/[A]₀ + kt

k = Ae^(-Ea/RT)
ln(k₂/k₁) = -Ea/R (1/T₂ - 1/T₁)
t₁/₂ = ln(2)/k (first order)

Equilibrium

Kc = [products]/[reactants]
Kp = Kc(RT)^Δn
ΔG° = -RT ln(K)
Kw = [H⁺][OH⁻] = 1.0 × 10⁻¹⁴

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