In this section, you will use evidence to explain the effects of changing the temperature or concentration of chemical reaction rates, including the idea that as the kinetic energy of colliding particles increases and the number of collisions increases, the reaction rate increases.

Answer 1

When the temperature or concentration of a reactant is increased in a chemical reaction, the kinetic energy of the particles involved also increases. This increase in kinetic energy means that the particles move faster and with more energy, leading to more frequent and energetic collisions between them.

According to the collision theory of chemical reactions, for a reaction to occur, the reacting particles must collide with enough energy and in the correct orientation. Increasing the temperature or concentration of reactants increases the likelihood of successful collisions, as the particles have a higher chance of meeting the energy threshold for reaction.

Furthermore, the increase in temperature or concentration also leads to an increase in the number of collisions happening per unit time. This increase in the frequency of collisions further enhances the reaction rate, as there are more opportunities for successful collisions to occur.

In conclusion, as the kinetic energy of colliding particles increases and the number of collisions between reactant particles increases, the reaction rate of a chemical reaction also increases. This is due to the increase in successful collisions happening as a result of the higher energy and frequency of collisions, ultimately leading to a faster rate of reaction.