Chemical Kinetics - What is instantaneous rate of reaction?
Definition of instantaneous rate of reaction
Calculation of instantaneous rate of reaction
Example: Reaction A + B → C
Initial concentrations: [A]₀ = 0.1 M, [B]₀ = 0.2 M
Time taken for [C] to increase from 0.05 M to 0.15 M is 20 seconds
Calculate the instantaneous rate of reaction at t = 20 seconds
Equation for instantaneous rate of reaction:
Rate = -∆[A]/∆t = -∆[B]/∆t = ∆[C]/∆t
Units of instantaneous rate of reaction: M/s or mol/(L·s)
Collision Theory of Chemical Reactions
Introduction to collision theory
Fundamental concepts of collision theory:
Collision frequency
Activation energy
Orientation factor
Effective collision
Factors affecting the rate of collision:
Concentration of reactants
Temperature
Surface area
Presence of catalysts
Rate Law and Rate Constant
Introduction to rate law and rate constant
Definition of rate law and rate constant
Determining the rate law using the method of initial rates
Example: Reaction: A + B → C
Experimental data for initial rates at different reactant concentrations
Calculation of rate law and rate constant
Units of rate constant: M^(n-1)·s^(-1) for nth order reactions
Integrated Rate Laws - Zero Order Reactions
Overview of integrated rate laws
Integrated rate law for zero order reactions
Derivation of integrated rate law for zero order reactions
Half-life of zero order reactions
Example: Reaction A → products
Plotting concentration vs. time and determining the rate constant
Calculating the half-life of the reaction
Integrated Rate Laws - First Order Reactions
Integrated rate law for first order reactions
Derivation of integrated rate law for first order reactions
Half-life of first order reactions
Example: Reaction A → products
Plotting concentration vs. time and determining the rate constant
Calculating the half-life of the reaction
Connection between integrated rate laws and rate constants
Integrated Rate Laws - Second Order Reactions
Integrated rate law for second order reactions
Derivation of integrated rate law for second order reactions
Half-life of second order reactions
Example: Reaction A + B → products
Plotting concentration vs. time and determining the rate constant
Calculating the half-life of the reaction
Arrhenius Equation and Activation Energy
Introduction to Arrhenius equation
Derivation of Arrhenius equation
Importance of activation energy in chemical reactions
Calculation of activation energy using Arrhenius equation
Example: Reaction rate constant data at different temperatures
Plotting ln(k) vs. 1/T and determining Activation Energy (Ea)
Effect of Temperature on Reaction Rate
Influence of temperature on reaction rate
Effect of temperature on the rate constant
Activation energy and temperature dependence
Relationship between rate constant and temperature: Arrhenius equation
Example: Reaction rate constant at different temperatures
Calculation of activation energy and temperature dependence of rate constant
Catalysts and Reaction Rates
Introduction to catalysts
Definition and characteristics of catalysts
Types of catalysts: homogeneous and heterogeneous
Mechanism of catalysis
Effect of catalysts on reaction rates
Example: Catalyzed vs. uncatalyzed reactions
Comparison of reaction rates with and without a catalyst
Chemical Kinetics - What is instantaneous rate of reaction?
Definition of instantaneous rate of reaction
Calculation of instantaneous rate of reaction
Example: Reaction A + B → C
Initial concentrations: [A]₀ = 0.1 M, [B]₀ = 0.2 M
Time taken for [C] to increase from 0.05 M to 0.15 M is 20 seconds
Calculate the instantaneous rate of reaction at t = 20 seconds
Equation for instantaneous rate of reaction:
Rate = -∆[A]/∆t = -∆[B]/∆t = ∆[C]/∆t
Units of instantaneous rate of reaction: M/s or mol/(L·s)
Collision Theory of Chemical Reactions
Introduction to collision theory
Fundamental concepts of collision theory:
Collision frequency
Activation energy
Orientation factor
Effective collision
Factors affecting the rate of collision:
Concentration of reactants
Temperature
Surface area
Presence of catalysts
Rate Law and Rate Constant
Introduction to rate law and rate constant
Definition of rate law and rate constant
Determining the rate law using the method of initial rates
Example: Reaction A + B → C
Experimental data for initial rates at different reactant concentrations
Calculation of rate law and rate constant
Units of rate constant: M^(n-1)·s^(-1) for nth order reactions
Integrated Rate Laws - Zero Order Reactions
Overview of integrated rate laws
Integrated rate law for zero order reactions
Derivation of integrated rate law for zero order reactions
Half-life of zero order reactions
Example: Reaction A → products
Plotting concentration vs. time and determining the rate constant
Calculating the half-life of the reaction
Integrated Rate Laws - First Order Reactions
Integrated rate law for first order reactions
Derivation of integrated rate law for first order reactions
Half-life of first order reactions
Example: Reaction A → products
Plotting concentration vs. time and determining the rate constant
Calculating the half-life of the reaction
Integrated Rate Laws - Second Order Reactions
Integrated rate law for second order reactions:
$ \frac{1}{[A]} = kt + \frac{1}{{[A]_0}} $
Derivation of integrated rate law for second order reactions
Half-life of second order reactions:
$ t_{\frac{1}{2}} = \frac{1}{{k[A]_0}} $
Relationship between rate constant and reaction time
Example: Reaction A + B → products
Plotting concentration vs. time and determining the rate constant
Calculating the half-life of the reaction
Arrhenius Equation and Activation Energy
Introduction to Arrhenius equation
Derivation of Arrhenius equation:
$ k = Ae^{-\frac{Ea}{RT}} $
Importance of activation energy in chemical reactions
Calculation of activation energy using Arrhenius equation
Example: Reaction rate constant data at different temperatures
Plotting ln(k) vs. 1/T and determining Activation Energy (Ea)
Effect of Temperature on Reaction Rate
Influence of temperature on reaction rate
Effect of temperature on the rate constant
Activation energy and temperature dependence
Relationship between rate constant and temperature: Arrhenius equation
Example: Reaction rate constant at different temperatures
Calculation of activation energy and temperature dependence of rate constant
Catalysts and Reaction Rates
Introduction to catalysts
Definition and characteristics of catalysts
Types of catalysts: homogeneous and heterogeneous
Mechanism of catalysis
Effect of catalysts on reaction rates
Example: Catalyzed vs. uncatalyzed reactions
Comparison of reaction rates with and without a catalyst