1. Chemical Kinetics is the branch of chemistry dealing with reaction rates.
2. Rate of reaction is the change in concentration of reactants/products per unit time.
3. Units of rate: mol dm⁻³ s⁻¹.
4. Rate law relates reaction rate to reactant concentrations (Rate = K [A]^x [B]^y).
5. Order of reaction is the sum of exponents in the rate law.
6. Zero-order reactions: rate is independent of reactant concentration.
7. Elementary reaction is a single-step reaction.
8. Complex reaction occurs in two or more steps.
9. Reaction mechanism describes the path from reactants to products.
10. The slowest step is the rate-determining step.
11. Catalyst speeds up reaction without permanent chemical change.
12. Homogeneous catalysis: catalyst & reactants in same phase.
13. Heterogeneous catalysis: catalyst in different phase (usually solid).
14. Enzymes are biochemical catalysts, highly specific, speed up reactions.
15. Enzyme-substrate complex is an intermediate in enzyme catalysis.
16. Activation Energy (Ea) is the minimum energy for reactants to form products.
17. Collision Theory states reactions occur via effective molecular collisions.
18. Transition State is an unstable intermediate formed during reaction.
19. Positive catalyst lowers Ea and increases rate.
20. Negative catalyst (inhibitor) blocks collisions and decreases rate.
21. Auto catalysis: product acts as catalyst.
22. Acid-Base Catalysis involves H⁺ or OH⁻ ions.
23. Surface Area affects reaction rate (greater area = faster rate).
24. Temperature: higher T increases reaction rate.
25. Concentration: higher concentration increases reaction rate.
26. Homogeneous catalysis examples include acid-base catalysis and auto catalysis.
27. Heterogeneous catalysis examples include contact process and Haber process.
28. Enzyme Catalysis involves lock-and-key model and enzyme-substrate complex.
29. Factors influencing reaction rate include concentration, surface area, temperature, catalysts, and radiation.