Arrhenius equation, activation energy barrier, and catalyst effect on reaction rates.
Arrhenius Equation:
k = A · exp(-Ea / RT)
where k = rate constant, A = pre-exponential factor
Ea = activation energy, R = 8.314 J/mol·K, T = temperature
Rate Laws:
Zero Order: rate = k, [A] = [A]₀ - kt
First Order: rate = k[A], [A] = [A]₀·exp(-kt)
Second Order: rate = k[A]², 1/[A] = 1/[A]₀ + kt
Half-life:
Zero Order: t₁/₂ = [A]₀ / 2k
First Order: t₁/₂ = ln(2) / k
Second Order: t₁/₂ = 1 / (k[A]₀)
Catalyst Effect:
Ea' = Ea - ΔEa (lowers barrier, increases k)