Why does increasing the temperature of a reaction cause the reaction rate to increase?

The potential energy of each particle increases.

Increased energy enables more particles to collide.

More collisions occur because average particle speed decreases.

The average kinetic energy of the particles decreases.

The correct answer is "Increased energy enables more particles to collide."

Explanation:

The reaction rate is defined as the change in the concentration of one of the reagents or products, in a time interval in which the change takes place.

For a chemical reaction to take place, the molecules of the reagents must collide, and must also collide effectively. In other words, these shocks must be produced with sufficient energy so that they can break and form chemical bonds. In the crash there must be proper orientation.

When increasing the temperature, the molecules will possess greater kinetic energy, which is that energy related to the movement of the molecules. Consequently, these molecules will move faster. Thus, the possibility of colliding with another molecule increases significantly. In this way, the reaction rate increases.

So, the correct answer is "Increased energy enables more particles to collide."

The answer is (B).

As temperature increases, the number of high energy collisions increases. It is because of these collisions that a reaction will result.