Kinetics

• Collision Theory: Chemical reactions occur when particles of substances collide with energy greater than or equal to the activation energy and correct particle orientation.
• Reaction Conditions: Changing the conditions of a reaction can increase the likelihood of collisions occurring with sufficient energy to react and increase the reaction rate.
• Maxwell-Boltzmann Distribution: Not all molecules in a substance have the same amount of energy, and their energies are distributed in a pattern called the Maxwell-Boltzmann distribution.
• Effect of Temperature: Increasing the reaction temperature increases the rate of reaction as more collisions of greater energy occur.
• Effect of Concentration and Pressure: Increasing the concentration or pressure of a sample increases the rate of reaction by increasing the likelihood of collisions occurring with energy greater than the activation energy.