⚡ Chemical Reactions & Kinetics — Advanced#

Scope — Energy landscapes, transition state theory, catalysis, and quantitative modeling of reaction dynamics.

Key concepts#

• Activation energy — minimum energy barrier that must be overcome for a reaction to proceed.
• Transition state theory — describes reaction rates in terms of activated complexes at energy maxima.
• Catalysis — acceleration of reactions by lowering activation energy without being consumed.

Seed Q&A triads#

• Q: How does a catalyst increase reaction rate without changing equilibrium?
  A: It provides an alternative pathway with lower activation energy, speeding both forward and reverse reactions equally.

• Q: What information does an energy profile diagram convey?
  A: Relative energies of reactants, products, intermediates, and transition states along the reaction coordinate.

• Q: How does temperature quantitatively affect reaction rate?
  A: Through the Arrhenius equation, where rate increases exponentially with temperature due to more molecules exceeding activation energy.

Contributor prompts and extensions#

• Add a worked example using the Arrhenius equation to calculate activation energy from experimental data.
• Include a comparison of homogeneous vs heterogeneous catalysis with real‑world examples.
• Discuss how kinetic control differs from thermodynamic control in product formation.

Advanced exercises#

• Analyze how changing catalyst concentration affects rate but not equilibrium position.
• Interpret experimental data to distinguish between competing reaction mechanisms.