According to the collision theory and model created to explain the collision theory, what is the best explanation for why a higher temperature makes a reaction go faster?

1. there are more collisions per miute

2. it increases the distance between the particles

3. it increases the average kinetic energy of the particles

4. it increases the average kinetic energy and there are more collisions per minute

Question

Ann Boyd

Chemistry

20 November, 17:48

According to the collision theory and model created to explain the collision theory, what is the best explanation for why a higher temperature makes a reaction go faster?

1. there are more collisions per miute

2. it increases the distance between the particles

3. it increases the average kinetic energy of the particles

4. it increases the average kinetic energy and there are more collisions per minute

+1

Answers (2)

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Douglas Smith · Answer 1

Answer is: 4. it increases the average kinetic energy and there are more collisions per minute.

The average kinetic energy of molecules depends on the temperature.

As temperature increases, molecules gain more energy from surrounding and move faster and have more collisions.

Kinetic energy (standard unit is the joule J) depends on speed of the molecule.

The collision theory states that when suitable particles of the reactant hit each other, only a certain fraction of the collisions cause any noticeable or significant chemical change. These successful changes are called successful collisions.

Fitzpatrick · Answer 2

4. it increases the average kinetic energy and there are more collisions per minute.