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the result should be reactants going to products because think of it this way.
Every reaction has a minimum energy requirement, that's required to go from reactants to products. that's the point of a reaction; you put in energy molecules collide, go through a transition state, and you get products.
In Arrhenius theory it says:
1) For a reaction to occur there should be reactant molecules as well as collisions between reactant molecules.
2) The collisions between reactant molecules should occur in favourable orientations.
3) The reactant molecules that collide with the perfect orientation should have the necessary activation energy.
A collision that meets the above requirements is termed as an effective collision.
So I guess it says it all. When there's effective collisions there would be a reaction with the reactants to form products. Basically the rate of reaction is depends upon the effective collisions.