''The rate a reaction is proportional to the number of effective collisions occurring per second between the reactants''. This statement is associated with ...

The statement "The rate a reaction is proportional to the number of effective collisions occurring per second between the reactants" is associated with Collision Theory. Collision theory explains how chemical reactions occur at the molecular level. It states that for a reaction to occur, the reacting molecules must collide with each other with sufficient energy and proper orientation. Not all collisions lead to a reaction, only those with enough energy and correct orientation can lead to a successful reaction. The rate of a reaction is determined by the frequency of these effective collisions. The more frequently the reactant molecules collide with enough energy and proper orientation, the faster the reaction rate. Therefore, the statement emphasizes that the rate of a chemical reaction is proportional to the number of successful collisions (effective collisions) occurring between the reactants per second.