6.2.2 — Collision Theory
Paper 4 · 15 Questions · 24 Marks · Core Level
Define the term activation energy.
Which of the following best describes activation energy?
A reaction has a high activation energy. Explain what this means in terms of particle collisions.
True or False: Activation energy is the energy released by a reaction.
On an energy profile diagram, where is the activation energy measured FROM and TO?
Explain why not all collisions between reactant particles result in a chemical reaction.
Which condition must be met for a collision to be SUCCESSFUL (i.e., lead to a reaction)?
Two particles collide but no reaction occurs. Using the concept of activation energy, explain this observation.
True or False: Every collision between reactant particles results in a chemical reaction.
At room temperature, hydrogen and oxygen gas can coexist in a container without reacting. Explain this in terms of collision theory.
What is meant by the 'frequency of collisions'?
Increasing the concentration of a reactant increases the rate of reaction. Explain this in terms of collision frequency.
Which change would DIRECTLY increase the frequency of collisions between reactant particles?
A student increases the temperature of a reaction. State TWO reasons, in terms of collision theory, why the rate of reaction increases.
A solid reactant is ground into a fine powder before being used in a reaction. Explain how this increases the rate of reaction using collision theory.
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