Chemical Kinetics- Potential Energy diagram and transition state

  • Rate of a reaction
  • Collision theory
  • Activation energy
  • Potential energy diagram
  • Transition state theory Example: Consider the reaction: A + B → C Equation: Rate = k[A][B] (END SLIDE 1)

Rate of Reaction

  • Definition of rate of reaction
  • Factors affecting the rate of reaction
    • Concentration
    • Temperature
    • Catalysts
    • Surface area
  • Rate expression Example:

2A + B → 3C Rate = k[A]^2[B] (END SLIDE 2)

Collision Theory

  • Definition of collision theory
  • Factors affecting collision frequency
    • Concentration
    • Temperature
    • Surface area
  • Effective collision
  • Activation energy Example: A + B → C (END SLIDE 3)

Activation Energy

  • Definition of activation energy
  • Role in a chemical reaction
  • Effect of temperature on activation energy
  • Maxwell-Boltzmann distribution Example: Reaction: A + B → C Activation energy: Ea (END SLIDE 4)

Potential Energy Diagram

  • Introduction to potential energy diagrams
  • Representation of energy changes in a reaction
  • Exothermic and endothermic reactions
  • Activation energy on potential energy diagram Example: Potential energy diagram for the reaction: A + B → C (END SLIDE 5)

Reaction Mechanisms

  • Multistep reactions
  • Elementary steps
  • Rate-determining step
  • Intermediates Example: Reaction mechanism of the decomposition of hydrogen peroxide (END SLIDE 6)

Order and Molecularity

  • Definition of order of reaction
  • Determination of order from rate equation
  • Molecularity of a reaction
  • Unimolecular, bimolecular, and termolecular reactions Example: Rate = k[A]^2[B]^3 Order of reaction: 2+3 = 5 (END SLIDE 7)

Rate Law and Rate Constant

  • Derivation of rate law
  • Determination of rate constant
  • Relationship between rate constant and rate equation
  • Units of rate constant Example: Rate = k[A][B]^2 Rate constant: k (END SLIDE 8)

Integrated Rate Laws

  • Zero-order reactions and integrated rate equation
  • First-order reactions and integrated rate equation
  • Half-life and its significance
  • Second-order reactions and integrated rate equation Example: Zero-order reaction: A → B Rate = k (END SLIDE 9)

Collision Theory and Transition State Theory

  • Comparison between collision theory and transition state theory
  • Role of transition state in a chemical reaction
  • Activation energy in transition state theory Example: Transition state theory for the reaction: A + B → C (END SLIDE 10)

Collision Frequency

  • Definition of collision frequency
  • Relationship between collision frequency and concentration
  • Relationship between collision frequency and temperature
  • Relationship between collision frequency and surface area
  • Effective collision and its importance Example:
  • Collisions between reactant molecules A and B
  • Increasing concentration of A and B leads to a higher collision frequency

Activation Energy and Reaction Rate

  • Explanation of activation energy
  • Relationship between activation energy and reaction rate
  • Effect of temperature on reaction rate
  • Arrhenius equation
  • Calculation of activation energy using Arrhenius equation Example:
  • Activation energy and the height of the energy barrier on the potential energy diagram

Catalysts and Reaction Rate

  • Definition of catalysts
  • Mechanism of catalysis
  • Role of catalysts in lowering activation energy
  • Difference between homogeneous and heterogeneous catalysis
  • Examples of catalysts in industrial and biological processes Example:
  • Enzymes as biological catalysts in living organisms

Rate-Determining Step

  • Definition of rate-determining step
  • Identification of rate-determining step in reaction mechanisms
  • Influence of rate-determining step on overall reaction rate
  • Role of intermediates in rate-determining step
  • Factors affecting the rate-determining step Example:
  • Rate-determining step in the reaction mechanism of the Haber process

Order of Reactions

  • Definition of order of reaction
  • Determination of order from experimental data
  • Relationship between order and rate equation
  • Difference between overall order and individual orders
  • Examples of reactions with different orders Example:
  • First-order reaction: A → B

First-Order Reactions

  • Integrated rate equation for first-order reactions
  • Calculation of reaction rate from integrated rate equation
  • Half-life and its significance in first-order reactions
  • Unit of rate constant for first-order reactions
  • Examples of first-order reactions Example:
  • Decay of radioactive isotopes

Second-Order Reactions

  • Integrated rate equation for second-order reactions
  • Calculation of reaction rate from integrated rate equation
  • Half-life and its significance in second-order reactions
  • Unit of rate constant for second-order reactions
  • Examples of second-order reactions Example:
  • A + B → C (Second-order with respect to A and B)

Zero-Order Reactions

  • Integrated rate equation for zero-order reactions
  • Calculation of reaction rate from integrated rate equation
  • Half-life and its significance in zero-order reactions
  • Unit of rate constant for zero-order reactions
  • Examples of zero-order reactions Example:
  • Decomposition of hydrogen peroxide in the presence of a catalyst

Effect of Temperature on Reaction Rate

  • Relationship between temperature and reaction rate
  • Activation energy and its effect on the temperature dependence of reaction rate
  • Collision theory and temperature dependence
  • Arrhenius equation and its application to temperature dependence
  • Examples illustrating the effect of temperature on reaction rate Example:
  • Effect of increasing temperature on the reaction rate of the combustion of methane

Catalysts and Reaction Rate

  • Definition of catalysts
  • Mechanism of catalysis
  • Role of catalysts in lowering activation energy
  • Difference between homogeneous and heterogeneous catalysis
  • Examples of catalysts in industrial and biological processes Example:
  • Enzymes as biological catalysts in living organisms (END SLIDE 21)

Rate-Determining Step

  • Definition of rate-determining step
  • Identification of rate-determining step in reaction mechanisms
  • Influence of rate-determining step on overall reaction rate
  • Role of intermediates in rate-determining step
  • Factors affecting the rate-determining step Example:
  • Rate-determining step in the reaction mechanism of the Haber process (END SLIDE 22)

Order of Reactions

  • Definition of order of reaction
  • Determination of order from experimental data
  • Relationship between order and rate equation
  • Difference between overall order and individual orders
  • Examples of reactions with different orders Example:
  • First-order reaction: A → B (END SLIDE 23)

First-Order Reactions

  • Integrated rate equation for first-order reactions
  • Calculation of reaction rate from integrated rate equation
  • Half-life and its significance in first-order reactions
  • Unit of rate constant for first-order reactions
  • Examples of first-order reactions Example:
  • Decay of radioactive isotopes (END SLIDE 24)

Second-Order Reactions

  • Integrated rate equation for second-order reactions
  • Calculation of reaction rate from integrated rate equation
  • Half-life and its significance in second-order reactions
  • Unit of rate constant for second-order reactions
  • Examples of second-order reactions Example:
  • A + B → C (Second-order with respect to A and B) (END SLIDE 25)

Zero-Order Reactions

  • Integrated rate equation for zero-order reactions
  • Calculation of reaction rate from integrated rate equation
  • Half-life and its significance in zero-order reactions
  • Unit of rate constant for zero-order reactions
  • Examples of zero-order reactions Example:
  • Decomposition of hydrogen peroxide in the presence of a catalyst (END SLIDE 26)

Effect of Temperature on Reaction Rate

  • Relationship between temperature and reaction rate
  • Activation energy and its effect on the temperature dependence of reaction rate
  • Collision theory and temperature dependence
  • Arrhenius equation and its application to temperature dependence
  • Examples illustrating the effect of temperature on reaction rate Example:
  • Effect of increasing temperature on the reaction rate of the combustion of methane (END SLIDE 27)

Factors Affecting Reaction Rate

  • Concentration and reaction rate
    • Rate law
    • Rate constant
  • Temperature and reaction rate
    • Activation energy
    • Arrhenius equation
  • Catalysts and reaction rate
  • Surface area and reaction rate Example:
  • Effect of increasing reactant concentration on reaction rate (END SLIDE 28)

Kinetics vs. Thermodynamics

  • Difference between kinetics and thermodynamics
  • Focus of kinetics on reaction rates and mechanisms
  • Focus of thermodynamics on energy changes and equilibrium
  • Relationship between kinetics and thermodynamics in determining feasibility of reactions
  • Examples illustrating the interplay between kinetics and thermodynamics Example:
  • Exothermic reaction that is kinetically slow but thermodynamically favorable (END SLIDE 29)

Applications of Chemical Kinetics

  • Industrial applications of chemical kinetics
    • Production of chemicals
    • Pharmaceutical industry
  • Biological applications of chemical kinetics
    • Enzymatic reactions
    • Metabolic processes
  • Environmental applications of chemical kinetics
    • Reaction rates in the atmosphere
    • Decomposition of pollutants Example:
  • Use of chemical kinetics to optimize the production of a pharmaceutical drug (END SLIDE 30)