What happens to the average kinetic energy of reactants when temperature increases?

When the temperature of a system increases, the average kinetic energy of the reactant molecules also increases. This is due to the fact that temperature is a measure of the average kinetic energy of the particles in a substance.

As the kinetic energy rises, molecules move faster. This increase in speed results in more frequent and more forceful collisions between reactant particles. For chemical reactions to occur, reactants must collide with sufficient energy and proper orientation. Therefore, by increasing the chances of successful collisions, the likelihood of reactions taking place also increases, which can lead to a higher reaction rate.

In systems affecting reactions, this principle applies to all states of matter, not just gases, as kinetic energy influences the motion of particles regardless of whether they are solid, liquid, or gas. Thus, the correct choice highlights the connection between temperature, kinetic energy, and the dynamics of chemical reactions effectively.