Collision Theory & Reaction Rates

These flashcards cover key concepts and definitions related to collision theory and factors affecting reaction rates.

Collision Theory

Molecules must collide with enough energy and in the correct orientation in order to react.

Activation Energy (EA)

The energy required to break bonds during a chemical reaction.

Reaction Rate

The speed at which a chemical reaction occurs, influenced by factors such as collisions.

Successful Collision

A collision between molecules that results in a reaction.

Temperature Effect on Reaction Rate

Increasing temperature increases kinetic energy of particles, leading to more collisions and faster reaction rates.

Concentration Effect on Reaction Rate

Increasing concentration raises the number of particles in a unit volume, leading to more collisions and faster reaction rates.

Catalyst

A substance that increases the rate of a reaction by lowering the activation energy required for the reaction.

Surface Area Effect on Reaction Rate

Increasing surface area (by decreasing particle size) leads to more collisions and faster reaction rates.