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:
- [A]1=kt+[A]01
- Derivation of integrated rate law for second order reactions
- Half-life of second order reactions:
- t21=k[A]01
- 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−RTEa
- 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)