Chapter 9. Chemical Kinetics
Rate law: rate = k[A]ᵐ[B]ⁿ, where orders m and n are found experimentally, not from coefficients [2].
| Order | Integrated law | Half-life |
| 0 | [A] = [A]₀ − kt | [A]₀/2k |
| 1 | ln[A] = ln[A]₀ − kt | 0.693/k |
| 2 | 1/[A] = 1/[A]₀ + kt | 1/k[A]₀ |
Collision theory and Arrhenius equation: k = A e^(−Eₐ/RT). Higher temperature, lower activation energy, and catalysts all increase rate; a catalyst provides a new pathway with lower Eₐ without being consumed [4][5].
Mechanisms are sequences of elementary steps; the slowest is the rate-determining step.
Review: A first-order reaction has k = 0.0231 min⁻¹. What is its half-life? (30 min.)