Chemical Kinetics- - Closer Look At Chemical Reaction Process

Slide 3

Collision Theory of Chemical Reactions
Successful collision and activation energy
Role of effective collisions in reaction rate
Activation energy and reaction barriers

Slide 4

Rate of Reaction: Average Rate
Definition and calculation of average rate of reaction
Units of rate of reaction
Determination of reaction rate using changes in concentration

Slide 5

Rate of Reaction: Instantaneous Rate
Definition and calculation of instantaneous rate of reaction
Determination of reaction rate using rate expression

Slide 6

Integrated Rate Laws
Zero-Order Reactions
First-Order Reactions
Second-Order Reactions

Slide 7

Determination of Order of Reaction
Graphical Method
Method of Initial Rates

Slide 8

Half-Life of Reactions
Definition and calculation of half-life
Relationship between half-life and reaction order

Slide 9

Rate-Determining Step
Definition and importance of rate-determining step
Concept of elementary steps and rate laws

Slide 10

Collision Theory and Reaction Mechanisms
Concept of reaction mechanism
Role of intermediates and catalysts
Relationship between reaction mechanism and rate law

Slide 11

Rate Laws and Rate Constants
- Rate law expression and rate constant
  - k, the rate constant
- Relationship between rate law and reaction order
First-Order Reactions
- Rate law expression for first-order reactions
  - Rate = k[A]
- Half-life of first-order reactions
  - t1/2 = 0.693/k
Second-Order Reactions
- Rate law expression for second-order reactions
  - Rate = k[A]^2 or Rate = k[A][B]
- Half-life of second-order reactions
  - t1/2 = 1/(k[A]0)
Zero-Order Reactions
- Rate law expression for zero-order reactions
  - Rate = k
- Half-life of zero-order reactions
  - t1/2 = [A]0 / 2k

Slide 12

Temperature and Rate Constant
- Effect of temperature on reaction rate
  - Increasing temperature increases rate of reaction
- Activation energy and Arrhenius equation
  - The role of activation energy in reaction rate
  - Arrhenius equation: k = A * e^(-Ea/RT)
    - k is the rate constant
    - A is the pre-exponential factor
    - Ea is the activation energy
    - R is the gas constant
    - T is the temperature in Kelvin

Slide 13

Reaction Mechanisms
- Multistep Reactions
- Reaction intermediates and rate-determining step
- Overall rate law and elementary steps
- Rate expression for each step and overall rate expression
Elementary Reactions
- Definition and characteristics of elementary reactions
- Unimolecular Reactions (A → products)
- Bimolecular Reactions (A + B → products)
- Termolecular Reactions (A + B + C → products)

Slide 14

Catalysts and Reaction Rate
- Definition and role of catalysts in chemical reactions
- Catalysts and reaction mechanism
- Heterogeneous catalysts and surface reactions
- Enzymes and biological catalysts
Factors Influencing Reaction Rate
- Effect of concentration on reaction rate
- Effect of temperature on reaction rate
- Effect of catalyst on reaction rate

Slide 15

Rate Laws and Equilibrium Constants
- Relationship between rate constants and equilibrium constants
- Equilibrium constant expression and reaction quotients
- Relationship between forward and reverse rate constants
Reversible Reactions and Equilibrium
- Definition of reversible reactions
- Forward and reverse reaction rates
- Equilibrium position and dynamic equilibrium

Slide 16

Le Chatelier’s Principle
- Definition and statement of Le Chatelier’s Principle
- Predicting the effect of changes on equilibrium position
- Effect of temperature, pressure, and concentration changes
Factors Affecting Equilibrium Constants
- Effect of temperature on equilibrium constant
- Effect of pressure and volume on equilibrium constant
- Effect of changing concentrations on equilibrium constant

Slide 17

Solubility Equilibrium and Ksp
- Definition of solubility equilibrium
- Solubility product constant (Ksp)
  - Ksp expression and values
- Common ion effect and precipitation reactions
Acid-Base Equilibrium and Ka/Kb
- Definition of acid-base equilibrium
- Acid dissociation constant (Ka) and base dissociation constant (Kb)
  - Ka expression and values
  - Henderson-Hasselbalch equation

Slide 18

pH and pOH
- Definition and calculation of pH and pOH
- Relationship between pH and pOH
- Acidic, basic, and neutral solutions
Buffer Solutions
- Definition and characteristics of buffer solutions
- Buffer capacity and buffer range
- Henderson-Hasselbalch equation for buffer solutions

Slide 19

Solubility and Complexation Equilibria
- Solubility product constant (Ksp) and solubility
  - Calculating solubility from Ksp
  - Effect of pH on solubility
- Complexation equilibrium and stability constant (Kf)
  - Formation constant (Kf) expression and values
  - Determining the formation of complex ions

Slide 20

Redox Reactions and Electrochemical Cells
- Oxidation and reduction reactions
  - Redox equations and half-reactions
- Balancing redox reactions using the Half-Reaction Method
  - Steps for balancing redox reactions
  - Examples of balancing redox reactions
Electrochemical Cells
- Definition and components of electrochemical cells
- Anode, cathode, and salt bridge
- Cell potential, standard potential, and electrode potentials

Slide 21

Rate Determination and Rate Laws
- How to determine the rate law of a reaction
- Use of initial rates and rate constants
- Examples of rate determination using experimental data
Rate Laws and Rate Equations
- General form of rate equations
- Use of rate constants
- Relationship between concentrations and reaction rate
Rate Laws and Stoichiometry
- Effect of stoichiometry on rate laws
- Determination of reaction order
- Rate laws for complex reactions
Rate Expression and Rate Constants
- Rate expression as a function of reactant concentrations
- Determining rate constants from experimental data
Examples:
- Determination of rate law for a reaction: A + B -> C
- Calculation of rate constant from experimental data

Slide 22

Reaction Mechanisms and Elementary Steps
- Definition of reaction mechanisms
- Elementary steps and overall reaction
- Role of intermediates in reaction mechanisms
Reaction Mechanism and Rate Determining Step
- Rate determining step and overall reaction rate
- Rate law expression for overall reaction
- Examples of reaction mechanisms and rate determining steps
Reaction Mechanism and Activation Energy
- Relationship between reaction mechanism and activation energy
- Energy profile diagram for a reaction
- Role of transition states in reaction mechanism
Examples:
- Reaction mechanism of nitric oxide formation
- Rate determining step in the combustion of methane

Slide 23

Reaction Order and Rate Constants
- Determination of reaction order from rate equation
- Relationship between reaction order and rate constants
- Examples of reaction order determination
Rate Laws and Temperature
- Effect of temperature on rate constants
- Arrhenius equation and activation energy
- Calculation of rate constants at different temperatures
Collision Theory and Activation Energy
- Basic principles of collision theory
- Effect of activation energy on reaction rate
- Relationship between activation energy and rate constant
Examples:
- Calculation of rate constant at different temperatures using Arrhenius equation
- Determination of activation energy from experimental data

Slide 24

Catalysts and Reaction Rates
- Definition and role of catalysts in reactions
- Types of catalysts: homogeneous and heterogeneous
- Effect of catalyst on activation energy and reaction rate
Factors Affecting Reaction Rates
- Concentration of reactants
- Temperature of the reaction
- Presence of catalysts
- Surface area of the reactants
Catalytic and Non-catalytic Reactions
- Comparison between catalytic and non-catalytic reactions
- Examples of catalytic reactions in industry and everyday life
Examples:
- Effect of catalyst on reaction rate: decomposition of hydrogen peroxide
- Influence of reactant concentration on reaction rate: iodine clock reaction

Slide 25

Rate Laws, Equilibrium Constants, and Le Chatelier’s Principle
- Relationship between rate constants and equilibrium constants
- Equilibrium position and reaction rates
- Le Chatelier’s Principle and its application to reaction rates
Reversible Reactions and Equilibrium
- Definitions of reversible reactions and equilibrium
- Forward and reverse reaction rates at equilibrium
- Calculation of equilibrium constant from reaction rates
Solubility Equilibrium and Ksp
- Definition of solubility equilibrium
- Solubility product constant (Ksp) and its calculation
- Common ion effect on solubility equilibrium
Examples:
- Calculation of equilibrium constant from reaction rates
- Determination of solubility product constant for a salt

Slide 26

Acid-Base Equilibrium and Ka/Kb
- Acid dissociation constant (Ka) and base dissociation constant (Kb)
- Calculation of Ka/Kb from acid/base concentrations
- Relationship between Ka and acid strength, and between Kb and base strength
pH and pOH
- Definition and calculation of pH and pOH
- Relationship between pH, pOH, and concentration of H+ and OH- ions
- Acidity and basicity of solutions based on pH values
Buffer Solutions
- Definition and characteristics of buffer solutions
- Buffer capacity and buffer range
- Henderson-Hasselbalch equation for buffer solutions
Examples:
- Calculation of pH and pOH of acidic and basic solutions
- Preparation of buffer solutions and determination of their pH

Slide 27

Solubility and Complexation Equilibria
- Solubility product constant (Ksp) and its calculation
- Calculation of solubility from Ksp values
- Effect of pH on solubility equilibrium
Complexation Equilibrium and Stability Constant
- Formation of complex ions and equilibrium constant (Kf)
- Calculation of formation constant from reactant concentrations
- Determination of the formation of complex ions in a reaction
Redox Reactions and Electrochemical Cells
- Oxidation and reduction reactions
- Balancing redox reactions using the Half-Reaction Method
- Electrochemical cells and cell potentials
Examples:
- Calculation of solubility from Ksp values
- Balancing redox reactions using the Half-Reaction Method

Slide 28

Factors Affecting Equilibrium Constants
- Effect of temperature on equilibrium constant
- Effect of changing concentrations on equilibrium constant
- Effect of pressure and volume changes on equilibrium constant
Solubility Equilibrium and Common Ion Effect
- Definition of solubility equilibrium
- Common ion effect on solubility of salts
- Calculation of solubility considering the common ion effect
Le Chatelier’s Principle
- Definition and statement of Le Chatelier’s Principle
- Predicting the effect of changes on equilibrium position
- Examples of applying Le Chatelier’s Principle
Examples:
- Calculation of equilibrium constant considering temperature changes
- Application of Le Chatelier’s Principle to predict equilibrium shift

Slide 29

Redox Reactions and Half-Cell Potentials
- Definition of half-cell potentials and standard potentials
- Calculation and determination of half-cell potentials
- Electrochemical series and predicting redox reactions
Oxidation-Reduction Titrations
- Definition and process of oxidation-reduction titrations
- Examples of oxidation-reduction titrations
- Calculation of unknown concentration using redox titration data
Electromotive Force (EMF) and Nernst Equation
- Definition of electromotive force (EMF)
- Nernst equation and its application to calculate cell potential
- Relationship between cell potential and Gibbs free energy change
Examples:
- Determination of half-cell potentials and predicting redox reactions
- Calculation of cell potential and Gibbs free energy change using Nernst equation

Slide 30

Biochemical Reactions and Enzymes
- Definition and types of biochemical reactions
- Role of enzymes as biological catalysts
- Enzyme-substrate complex and enzyme specificity
Factors Affecting Biochemical Reactions
- Effect of temperature and pH on enzymatic activity
- Enzyme inhibitors and their impact on reaction rate
- Use of enzyme kinetics to study biochemical reactions
Examples:
- Enzyme-catalyzed reactions in metabolism
- Influence of temperature and pH on enzymatic activity