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Rates of ReactionIntroduction

The Chemistry of Speed

Part of Rates & Collision Theory — GCSE Chemistry

This introduction covers The Chemistry of Speed within Rates & Collision Theory for GCSE Chemistry. Revise Rates & Collision Theory in Rates of Reaction for GCSE Chemistry with 20 exam-style questions and 16 flashcards. This is a high-frequency topic, so it is worth revising until the explanation feels precise and repeatable. It is section 1 of 13 in this topic. Use this introduction to connect the idea to the wider topic before moving on to questions and flashcards.

Topic position

Section 1 of 13

Practice

20 questions

Recall

16 flashcards

📖 The Chemistry of Speed

Some reactions happen in an instant — an explosion, a firework, a neutralisation. Others take years — iron rusting, rocks weathering, wine maturing. But what makes one reaction lightning-fast while another crawls along? The answer lies in something beautifully simple: collisions. For a reaction to happen, particles must collide with enough energy AND in the right orientation. The rate of reaction depends on how often these "successful collisions" occur. Understanding this lets us control chemistry — speeding up industrial processes, slowing down food spoilage, and optimising everything from medicine to manufacturing.
🎱 The Pool Table Analogy

Reactions are like potting balls in pool! Particles must collide (balls must hit) with enough energy (hard enough) AND at the right angle (correct aim) for a successful pot. More balls on the table = more collisions = more chances to score. This is collision theory — successful reactions need enough energy AND the right orientation!

Keep building this topic

Read this section alongside the surrounding pages in Rates & Collision Theory. That gives you the full topic sequence instead of a single isolated revision point.

Collision Theory — Temperature EffectDeep Dive: Collision TheoryHow Collision Theory Explains Rate

Practice Questions for Rates & Collision Theory

According to collision theory, which of the following must happen for a chemical reaction to take place?

  • A. Particles must dissolve in water
  • B. Particles must collide with sufficient energy
  • C. Particles must be heated to 100 degrees C
  • D. Particles must be in the liquid state
1 markfoundation

Explain, using collision theory, why increasing the concentration of a reactant solution increases the rate of reaction.

2 marksstandard

Quick Recall Flashcards

What is rate of reaction?
How quickly reactants are used up or products are formed
What are the units for rate?
g/s, cm³/s, or mol/s

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Collision Theory — Temperature Effect