3.x Collision Theory (GCSE Chemistry)

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

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

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

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

According to collision theory, ineffective collisions are due to:

Activation energy is precisely defined as:

Why does increasing temperature generally speed up a chemical reaction?

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

What happens to collision frequency when concentration of reactants decreases, according to collision theory?

What is defined by collision theory?

According to collision theory, to double the rate of reaction you would typically:

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

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