In this section, you will evaluate evidence to explain how increasing the temperature of reactants causes an increase in the rate of a chemical reaction.

Answer 1

When the temperature of reactants is increased, it leads to a greater amount of kinetic energy in the molecules. This increased energy causes the molecules to collide more frequently and with greater force, leading to an increased likelihood of successful collisions that result in a reaction.

According to the collision theory, for a chemical reaction to occur, reactant molecules must collide with sufficient energy and in the correct orientation. Increasing the temperature of the reactants increases the average kinetic energy of the molecules, which in turn increases the likelihood of successful collisions by providing them with the necessary energy to overcome the activation energy barrier.

Additionally, an increase in temperature also leads to an increase in the number of high-energy collisions between molecules. These high-energy collisions are more likely to result in a reaction because the molecules involved have sufficient energy to break existing bonds and form new ones, leading to a faster overall reaction rate.

In summary, increasing the temperature of reactants increases the rate of a chemical reaction by providing molecules with more kinetic energy, leading to an increased frequency of collisions and a higher likelihood of successful reactions through high-energy collisions.