Reaction Kinetics — A/L Chemistry

Reaction kinetics governs the empirical rate of chemical transformations and the energetic pathway (activation energy Ea and rate equation R = k[A]^m[B]ⁿ) of multi-step reaction mechanisms.

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1. Order vs Stoichiometry: Proof that reaction order (m, n) is experimentally determined and cannot be deduced from overall stoichiometric coefficients.
2. Arrhenius Parameters: Accurate derivation of activation energy (Ea) from the slope (-Ea/R) of linear ln(k) vs 1/T graphs.
3. Rate-Determining Step: Mechanistic alignment proving the empirical rate law reflects only species involved up to and including the slowest (rate-determining) elementary step.