8.2Effect of Temperature on Reaction Rates & Activation Energy

These flashcards cover key concepts related to activation energy, Boltzmann distribution, and the effect of temperature on reaction rates.

What is activation energy (E)?

The minimum amount of energy that reactant particles need to overcome for a reaction to take place.

How does activation energy differ between exothermic and endothermic reactions?

In exothermic reactions, the activation energy is relatively small, while in endothermic reactions, it is relatively larger.

What is a Boltzmann distribution curve?

A graph that shows the distribution of energies among particles in a substance at a specific temperature.

What happens to the Boltzmann distribution curve when the temperature increases?

The curve flattens and the peak shifts to the right, indicating a greater proportion of particles have kinetic energy above the activation energy.

Why do particles need to collide in the correct orientation?

For a collision to be effective, reactant particles must collide with the correct orientation and possess a minimum energy equal to the activation energy.

What effect does increasing temperature have on reaction rates?

It increases the rate of reaction due to more effective collisions and a greater proportion of molecules having kinetic energy greater than the activation energy.

Why is the increase in the proportion of molecules above activation energy significant?

It has a greater effect on the rate of reaction than the increase in effective collisions.