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Topic Notes · Easy summaries with diagrams
Chapter 17 — Chapter 17 — Reaction Kinetics
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📘Easy summary
Reactions occur when particles collide. Collision frequency: number of collisions per unit volume per unit time. Only successful (effective) collisions — with energy ≥ activation energy (Eₐ, minimum energy needed) and proper orientation — form products. Reactants climb the energy hill to an activated complex (transition state), which then breaks down into products. Rate is fastest at the start because reactant concentration is highest; it slows as reactants are used up (reactants ↓, products ↑).
⭐Key points
- Energy comes from KE of moving molecules (heat).
🔬Diagram
🌿Real-life example
Mixture of H₂ and O₂ needs a spark.
💡Exam tip
- Define Eₐ precisely.
✅Quick check
1. Collisions per unit volume:
2. E > Eₐ reaction is:
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