Chemistry: Chemical Kinetics

• Chemical kinetics is the study of the mechanisms ( how aa reaction proceeds) and the rate of chemical reactions.
• Mechanism is how a reaction converts reactants to products.
• Rate is how fast a reaction converts reactants to products.
• Collision Theory - for your reaction to occur, reactants must undergo effective collision.
• Requirements for a reaction to occur in collision theory are Sufficient Energy and proper orientation.
• Sufficient energy is needed to break and form bonds
• Proper orientation is for the particles to form the expected or target substance.

  
• Activated complex is an unstable structure
• Activated complex at transition state is old bonds are partially broken and new bonds are partially formed.
• Energy Diagram

  
• Factors that affect the rate of reaction are concentration, temperature, surface area, and catalyst.
• Rate of reaction is how fast the reaction converts reactants to products.
• Concentration is the amount of particles present.
• Concentration is when the greater the reactant concentration, moremore frequent collisions, faster reaction rate
• Temperature is the average kinetic energy of the particles in a substance.
• Increase in temperature , more active particles
• Surface area is exposed particles of solid reactants .
• Increase in surface area, the greater frequency of collision, faster reaction
• Catalyst is a substance that increases the rate of a reaction by lowering the activation energy by providing an alternative pathway for the reaction.
• Catalyst is an opposite of an inhibitor
• Inhibitor slows down the rate by blocking the usual pathway of a reaction, more frequent collision, and faster reaction
• Rate law is a mathematical expression that shows how reactant concentration affects the rate of reaction
• Order of reaction shows the magnitude of the effect of changes in a reactant concentration on the rate of the reaction
• Rate constant is a specific for a given reaction at a given temperature and pressure