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Chemistry

Example output

Reactions, equations and definitions, pulled from your notes and worksheets.

Source: chem-rates.jpg · handwritten

Summary

Your notes on reaction rates cover the four factors thoroughly, and collision theory is stated correctly. What's missing is the link between them — why each factor changes the rate is left implicit, which makes explain-questions harder than they need to be.

Collision theory

Particles must collide with sufficient energy and correct orientation to react.

Factors affecting rate

Temperature, concentration, surface area and catalysts — all listed, none explained in terms of collisions.

Key terms

Activation energypage 2
The minimum energy colliding particles need for a reaction to occur.
Catalystpage 3
A substance that speeds a reaction by lowering activation energy, without being consumed.
Rate of reactionpage 1
The change in concentration of a reactant or product per unit time.
What changes the rate
1
Temperature
More energy → more successful collisions.
2
Concentration
More particles per volume → more frequent collisions.
3
Catalyst
Lowers activation energy. Not consumed.

Flashcards

Why does temperature increase reaction rate?
Particles move faster, so collisions are more frequent and more exceed the activation energy.
Does a catalyst get used up?
No — it's regenerated, which is why small amounts work.
Why does powdering a solid speed up reaction?
Greater surface area means more particles exposed for collision.

Practice question

Increasing concentration speeds up a reaction because…

Pick an answer to see the reasoning.

Study plan

  1. 1
    Link each rate factor to collision theory explicitly
    20 min
  2. 2
    Sketch an energy profile with and without a catalyst
    15 min
  3. 3
    Six explain-the-rate practice questions
    20 min

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