#EnthalpyChangeAndActivationEnergy

#Chemistry

#ChemicalEnergetics

Introduction

• For atoms or particles to react with each other in a chemical system they must collide together

• A number of factors affect the success of a collision:

  • Energy

  • Orientation

  • Number of collisions per second - the frequency of collisions

What is activation energy?

• In terms of the energy of collisions, there is a minimum amount of energy required for a successful collision

  • A successful collision is where the particles in the reactant(s) are rearranged to form the products

• This minimum amount of energy is called the activation energy, Ea 

• Different reactions have different activation energies, depending on the chemical identities involved

• Reactions with higher activation energies require more energy to start than those with lower activation energies

What is enthalpy change?

• The transfer of thermal energy during a reaction is called the enthalpy change, ΔH, of the reaction. 

• ΔH is:

  • Positive for en endothermic reaction

  • Negative for an exothermic reaction

Reaction pathway diagrams

Exothermic reactions

• A reaction is exothermic when more energy is released forming new bonds for the products than absorbed breaking the bonds in the reactants

• So, the products have less energy than the reactants

  • This means that the change in energy is negative 

• Therefore, an exothermic reaction has a negative value for enthalpy, ΔH 

• The reaction pathway diagram for an exothermic reaction is:

Endothermic reactions

• A reaction is endothermic when more energy is absorbed breaking the bonds in the reactants than released forming new bonds for the products 

• So, the products have more energy than the reactants

  • This means that the change in energy is positive 

• Therefore, an endothermic reaction has a positive value for enthalpy, ΔH 

• The reaction pathway diagram for an endothermic reaction is: