9.1 Introduction to Kinetics

8.1 Kinetics and Equilibrium

Kinetics and Equilibrium – Facts and Definitions

9.A Kinetics - Collision Theory/Activation Energy

Rates of Reactions. Collision Theory/Activation Energy

Introduction to Kinetics

Kinetics is the study of rates mechanisms of chemical reactions.

Rate is the speed at which a reactions taking place.

Mechanism is a series of reactions that lead to a  final products of reaction.

Rate of reaction is the speed at which a chemical reaction or a physical change occurs.

Measuring rate can be done by a number of ways such as the number of moles of reactants consumed per unit time or the number of moles of product produced per unit time.

Collision theory states that for chemical reaction to occur between reactants, there must be active collisions between the reacting particles.

Effect of collision is when reacting particles collide with sufficient ( right amount of) kinetic energy and at the proper orientation ( angle).

– Rate of reaction depends on frequency (how often) of effective collisions occurring between particles.

– Any factor that can change the frequency of effective collisions between reacting particles will change the rate of that reaction.

Activation energy is the energy needed to start a chemical reaction. All chemical reactions both endothermic and exothermic, require some amount of activation energy. Any factor that can change the amount of activation energy for chemical reaction will change the rate of that reaction.

A catalyst is any substance that can increase the speed (rate) of a reaction by lowering the activation energy for that reaction. A catalyst provides an alternate pathway for a reaction to occur faster.