3.1.5 Kinetics

Collision Theory

States that particles must collide with energy greater than the activation energy for a reaction to occur.

Activation Energy

The minimum energy required for a reaction to start or occur.

Rate of Reaction

Influenced by temperature, concentration, pressure (in gases), catalysts, and surface area.

Maxwell-Boltzmann distribution of molecular energies

Shows the range of kinetic energies of particles in a gas and the fraction that can overcome activation energy for a reaction.

Effect of temperature on reaction rate

Increasing temperature increases the rate by providing more particles with energy greater than activation energy.

Effect of concentration & pressure

Increasing concentration (or pressure in gases) leads to more frequent successful collisions and a higher reaction rate.

Catalysts

Substances that increase the rate of reaction by providing an alternative pathway with lower activation energy.