Which statement explains why increasing the

temperature increases the rate of a chemical

reaction, while other conditions remain the same?

(1) The reacting particles have less energy and

collide less frequently.

(2) The reacting particles have less energy and

collide more frequently.

(3) The reacting particles have more energy and

collide less frequently.

(4) The reacting particles have more energy and

collide more frequently.

Answer: option (4) The reacting particles have more energy and

collide more frequently.

Explanation:

1) In order to a a reaction happen, the reactants must reach the activation energy, which is the energy needed to form the activated complex

2) Then, the higher the energy of the reactants, the less the gap between the energy of the reactants and the activation energy.

3) As per the collision theory, the reactant molecules must collide with energy at least enough as to reach the the activation energy.

4) The kinetic energy of the molecules is higher as higher is the temperature.

Then, you conclude that when you increase the temperature, the molecules will have more energy, will move faster, will collide with more energy, and will produce more effective collisions, which increases the rate of reaction.

The correct answer is 4.

With the rise of the temperature, the particles obtain enough energy (activation energy) to start moving; as they acquire more and more energy, they'll start colliding more frequently.

The other alternatives have no logical flow in them, as more energy has as consequence more movement, that is collision.