⚡ Chemical Reactions & Kinetics — Intermediate#

Scope — Rate laws, reaction order, mechanisms, and how experimental data reveal kinetic behavior.

Key concepts#

• Rate law — mathematical relationship between reaction rate and reactant concentrations.
• Reaction order — exponent of concentration terms in the rate law; determined experimentally.
• Reaction mechanism — stepwise sequence of elementary reactions describing how products form.

Seed Q&A triads#

• Q: How is reaction order determined?
  A: By measuring how changes in reactant concentration affect the reaction rate experimentally.

• Q: What is the difference between an elementary step and an overall reaction?
  A: An elementary step occurs in a single molecular event; the overall reaction summarizes all steps combined.

• Q: Why does the rate law not always match the stoichiometric coefficients?
  A: Rate laws depend on the mechanism and rate‑determining step, not the overall balanced equation.

Short exercises#

• Given experimental rate data, determine the rate law and overall reaction order.
• Identify the rate‑determining step in a simple multistep mechanism.