3.x Collision Theory (GCSE Chemistry)

The following is a GCSE Chemistry test covering '3.x Collision Theory'

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Question 1

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Collision theory explains that increasing the surface area of a reactant enhances reaction rate by:

What must particles possess in order to successfully react upon collision?

Why might a reaction rate decrease when pressure of gaseous reactants is lowered?

Activation energy is precisely defined as:

Why do reactions typically slow over time, according to collision theory?

What change to particle collisions occurs when reactant particles are heated?

With regards to collision theory, stirring a solution:

Reaction rates increase if reactants are in powder form rather than lumps because powders have:

Collision theory explains which requirement regarding reactant orientation?

Why does increasing temperature generally speed up a chemical reaction?

Which of these is directly proportional to the rate of reaction according to collision theory?

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