AQA · Chemistry · 8462
GCSE Chemistry: Collision theory and activation energy
The rate and extent of chemical change · AQA GCSE Chemistry (8462), specification point 4.6.1.3. Cards are generated from the exam board's own specification for "Collision theory and activation energy", and every card links back to the page it came from. Specification © AQA — used with attribution.
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What is activation energy?
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The minimum amount of energy that particles must have in order to react.
What two conditions must be met for reacting particles to react, according to collision theory?
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The particles must collide with each other, and they must collide with sufficient energy (at least the activation energy).
The minimum energy particles need to react is called the ?.
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activation energy
Why does increasing the concentration of a solution increase the rate of reaction?
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More particles per unit volume means collisions happen more frequently, so the rate increases.
Why does increasing the pressure of reacting gases increase the rate of reaction?
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The particles are closer together, so they collide more frequently.
Why does increasing the surface area of a solid reactant increase the rate of reaction?
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More particles are exposed, so collisions with the solid happen more frequently.
Give two reasons why increasing temperature increases the rate of reaction.
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Particles collide more frequently, and the collisions are more energetic (more particles have at least the activation energy).
How does temperature differ from concentration in its effect on collisions?
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Temperature increases both the frequency and the energy of collisions; concentration only increases the frequency of collisions.
Why do smaller pieces of a solid react faster than one large lump?
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Smaller pieces have a higher surface area to volume ratio, so more particles are exposed for collisions.
Cutting a reacting solid into smaller pieces increases its surface area to ? ratio.
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volume
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