Kinetics

• Activation energy: minimum amount of energies particles need to collide with for a successful reaction to occur
• Catalyst: a substance that increases that rate of reaction by providing an alternate reaction pathway that requires a lower activation energy and is unchanged by the reaction
• Collision theory: reactions will only take place if particles collide with sufficient energy and in the correct orientation
• Rate of reaction: the change in the amount of reactant or product over time
• What is the effect on increasing temperature on the maxwell-boltzman distribution?

  the graph will shift to the right and flatten as a greater proportion of molecules will have the sufficient kinetic energy to collide and have a successful reaction
• Dynamic equilibrium: A state of equilibrium in which the rate of forward and reverse reactions are equal. concentrations of products and reactants remain unchanged