Why does increasing the temperature of reactants lead to an increased rate of chemical reactions?

Increasing the temperature of reactants is known to enhance the rate of chemical reactions primarily because particles gain heat energy and move faster. When the temperature rises, the kinetic energy of the molecules involved in the reaction increases. This increased movement means that the particles collide more frequently and with greater energy.

In terms of collision theory, for a reaction to occur, reactant molecules must collide with sufficient energy to overcome the activation energy barrier. Higher temperatures result in a greater proportion of collisions having enough energy to lead to successful reactions.

This concept is fundamental in understanding how temperature influences reaction kinetics. The more productive collisions enable a faster transition from reactants to products, illustrating the direct correlation between temperature and reaction rates.