Kinetics

Kinetics is the study of the rates of chemical reactions and the factors that affect these rates. It involves analyzing the speed of reactions, understanding reaction mechanisms, and determining the conditions that optimize reaction yields.

The rate determining step is the slowest step of the reaction; most important factor influencing reaction rate

The more number of steps means that the reaction is a slower reaction.

The Collision Theory is how reactant particles must collide and have the following when doing so:

• Proper amount of energy

• Proper Orientation, or alignment

  • Only when particles collide, there will be an effective collision resulting in a reaction

Factors affecting the rate of reaction

• Nature of reactants

  • Ionic substances react faster

    • Smaller, less bonds to break; less steps

  • Covalent substances react slower

    • Larger, more bonds to break; more steps

• Concentration

  • The increase in concentration means the increase in the rate of reaction

  • This is due to a higher number of reactant particles coming into contact, resulting in more effective collisions per unit time.

• Pressure

  • Increase pressure means the increase in the rate of reaction

    • Only affects gases

  • Increasing pressure decreases the volume

  • Decrease space between particles, more collisions

• Temperature

  • Increase in temperature will increase the rate of reaction

  • Greater speed will have more total collisions

• Surface Area

  • Increase the surface area

    • Making smaller pieces

  • Increasing the rate of reaction

  • Increasing the surface area exposes more reactant particles to possible collisions

• Catalyst

  • Speeds up the reaction rate without changing the reactants and products

    • Provided a shortcut or alternative pathway

      Lowers the activation energy