CHEMICAL KINETICS

Chemical Kinetics

• Study of rates and mechanisms of chemical reactions.

• Crucial for understanding reactions vital to life.

Collision Theory

• Explains conditions for chemical reactions:

  • Reactant particles must collide.

  • Colliding particles must have sufficient energy.

Factors Affecting Reaction Rates

• Concentration of Reactants:

  • Increasing concentration increases reaction rate.

• Nature of Reactants:

  • Some reactants are more reactive than others; bond types affect reaction speed.

• Surface Area:

  • Smaller particles have greater surface areas, increasing collision frequency.

• Temperature:

  • Higher temperature increases kinetic energy, leading to more frequent collisions.

• Catalysts:

  • Substances that increase reaction rates without permanent change.

Rate of Reaction

• Rate defined as speed at which a reaction proceeds.

• Calculated using changes in concentration over time.

Integrated Rate Laws

• First-order reactions show rate proportionality to reactant concentration:

  • Example: $ext{Rate} = k[N_2O_5]$

• Rate of formation and decomposition are related; can be calculated from stoichiometry of the reaction.