Chemical Kinetics

Study of the rates of reactions and the steps by which the occur

Pertaining to a chemical process that absorbs heat energy and produces positive change in enthalpy

Pertaining to a chemical process that releases heat energy and produces a negative change in enthalpy

Particles must collide before they can react. However, a collision alone doesn’t guarantee a reaction

Be properly oriented for the necessary rearrangement of atoms and electrons

Be forceful enough/possess enough energy to form products. Reactions follow only forceful, oriented collisions

Minimum amount of kinetic energy that must be possessed by the colliding molecules before they react

Colliding reactants that form a theoretical, transitional structure between reactant and product

tell how fast reactions change into products

Nature of reactants, concentration, temperature, surface area, and presence of catalysts

This controls the rate of the reaction. Reactive substances react quickly and vice versa. Some noble gases never react or barely do. Another variable is combination, H and Cl under certain conditions react vigorously.

This increases the rate of a reaction. Varies from reaction to reaction, it could double or even quadruple the rate

Reaction rates double for every 10 C in temperature. Higher temperatures increase number of collisions and the force of collisions

If a substance is broken up into smaller pieces more surface area is exposed causing it to react faster.

A substance that changes a reaction rate without being permanently changed or consumed by the reaction. Has lower activation energy

A class of catalysts that are naturally occurring biological substances

in the same phase as the reactants or in solution with a reactant

a catalyst in a separate phase than the reactant

A substance used to reduce a catalysts undesirable effects.