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Collision theory states that in order for a reaction to occur, the molecules participating must collide with each other. The rate of the reaction depends on the frequency of the collisions. Transition state theory regards chemical reactions as a continuous change in the relative positions of molecules and their potential energies and explains the rate of a chemical reaction by assuming that there is a special kind of chemical equilibrium (quasi-state) between reactants in the reaction and their activated state.
If the rate of reaction only depends on how frequently the molecules collide with each other, then what is the point in differentiating zero, first, and second order reactions? My logic here is are these categorizations ways of labelling higher probability zones that they will collide more? Its hard to describe but how can you predict how frequently they will collide? Cause i thought it was only dependent on temperature
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