Collision Theory

 
7.4 Collision Theory
 
Introduction to Collision Theory
  • Collision theory is used to explain how the factors (size, concentration, temperature, catalyst and pressure) affect the rate of reaction.
  • Particles are constantly moving at random and collide with each other.
  • The collision theory states that a chemical reaction may occur from the collision of the particles.
  • However, not all collision causes a chemical reaction.
  • Only effective collisions cause a chemical reaction.
  • The condition for effective collision is  as follows;
    • Particles must collide in the correct orientation.
    • Particles must possess the energy equal or more than the activation energy.
 
Activation Energy
The minimum energy needed by reactant for a chemical reaction to occur.
 
Energy Profile Diagram
A diagram showing the change of energy in a chemical reaction.
 
The image is an infographic titled ‘Factors Affecting the Rate of Reaction.’ It features a semi-circular chart with five segments, each labeled with a different factor: ‘The concentration of the reactant’ ‘Size of the reactant,’ ‘Temperature of reaction,’ ‘Catalyst,’ and ‘Pressure’ At the center of the chart is an illustration of a person looking up and pointing. The Pandai logo is present on the left side of the image. The color scheme includes shades of blue and white.
 
Factors Affecting the Rate of Reaction
Factor Explaination
Size of the reactant
  • Size of reactant smaller.
  • Higher total exposed surface area.
  • Higher collision frequency.
  • Higher effective collision frequency.
  • Higher rate of reaction.
The concentration of the reactant
  • A higher concentration of liquid reactant.
  • A higher number of particles per unit volume.
  • Higher collision frequency.
  • Higher effective collision frequency.
  • Higher rate of reaction.
Temperature of reaction
  • A higher temperature of the reaction.
  • The higher kinetic energy of particles.
  • Higher collision frequency.
  • Higher effective collision frequency.
  • Higher rate of reaction.
Catalyst
  • Presence of catalyst.
  • Lowers activation energy of the chemical reaction.
  • Higher collision frequency.
  • Higher effective collision frequency.
  • Higher rate of reaction.
Pressure
  • The higher pressure of the reaction.
  • Higher collision frequency.
  • Higher effective collision frequency.
  • Higher rate of reaction.

 

Collision Theory

 
7.4 Collision Theory
 
Introduction to Collision Theory
  • Collision theory is used to explain how the factors (size, concentration, temperature, catalyst and pressure) affect the rate of reaction.
  • Particles are constantly moving at random and collide with each other.
  • The collision theory states that a chemical reaction may occur from the collision of the particles.
  • However, not all collision causes a chemical reaction.
  • Only effective collisions cause a chemical reaction.
  • The condition for effective collision is  as follows;
    • Particles must collide in the correct orientation.
    • Particles must possess the energy equal or more than the activation energy.
 
Activation Energy
The minimum energy needed by reactant for a chemical reaction to occur.
 
Energy Profile Diagram
A diagram showing the change of energy in a chemical reaction.
 
The image is an infographic titled ‘Factors Affecting the Rate of Reaction.’ It features a semi-circular chart with five segments, each labeled with a different factor: ‘The concentration of the reactant’ ‘Size of the reactant,’ ‘Temperature of reaction,’ ‘Catalyst,’ and ‘Pressure’ At the center of the chart is an illustration of a person looking up and pointing. The Pandai logo is present on the left side of the image. The color scheme includes shades of blue and white.
 
Factors Affecting the Rate of Reaction
Factor Explaination
Size of the reactant
  • Size of reactant smaller.
  • Higher total exposed surface area.
  • Higher collision frequency.
  • Higher effective collision frequency.
  • Higher rate of reaction.
The concentration of the reactant
  • A higher concentration of liquid reactant.
  • A higher number of particles per unit volume.
  • Higher collision frequency.
  • Higher effective collision frequency.
  • Higher rate of reaction.
Temperature of reaction
  • A higher temperature of the reaction.
  • The higher kinetic energy of particles.
  • Higher collision frequency.
  • Higher effective collision frequency.
  • Higher rate of reaction.
Catalyst
  • Presence of catalyst.
  • Lowers activation energy of the chemical reaction.
  • Higher collision frequency.
  • Higher effective collision frequency.
  • Higher rate of reaction.
Pressure
  • The higher pressure of the reaction.
  • Higher collision frequency.
  • Higher effective collision frequency.
  • Higher rate of reaction.