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 does increasing temperature generally speed up a chemical reaction?

According to collision theory, ineffective collisions are due to:

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

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

Collision theory explains which requirement regarding reactant orientation?

Collision theory states that when concentration increases:

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

With regards to collision theory, stirring a solution:

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

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

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