Factors-affecting-rates-of-chemical-reactions (1)

FACTORS AFFECTING RATES OF CHEMICAL REACTION

  • Rate of Reaction: Speed at which a chemical reaction occurs; can be fast or slow.

  • Collision Theory: Reactions occur when particles collide with enough energy.

    • Not all collisions lead to a reaction.

    • Effective collisions require:

      1. Minimum kinetic energy (Activation energy).

      2. Correct orientation during collision.

  • Activation Energy: Minimum energy needed to initiate a reaction (e.g., a lighter igniting wood).

FACTORS AFFECTING REACTION RATE

  1. Temperature: Higher temperature increases particle energy and speeds up reactions (e.g., spoiling food).

  2. Surface Area of Reactants: Smaller pieces have larger surface areas, increasing collision chances (e.g., powdered sugar vs. sugar cube).

  3. Concentration of Reactants: Higher concentration = more particles = more collisions.

  4. Presence of Catalyst: Speeds up reactions without being consumed by lowering activation energy (e.g., enzymes, catalytic converters).

  5. Pressure: Affects gas reactions only; higher pressure increases reaction rate.