Rate of reaction

• Factors affecting rate

  • Temperature
  • Surface area
  • Presence of catalysts
  • Pressure of reacting gases
  • Concentration of reactants
• Collision theory

  • The more frequent collisions there are, the faster the reaction.
• Activation energy

  • The minimum amount of energy required that particles need to react in order to break the bonds for the reaction to start.
• Catalyst

  • Catalysts increase the rate of reaction but are not used up during the reaction.
  • They allow us to carry out reactions without increasing temperature which saves money.
  • When a catalyst is present, the particles require less energy to cross the activation barrier.
• Reversible reaction

  • Products can reform to their original reactants.
• Equilibrium

  • In chemical reactions, a situation where the forward and backward reactions happen at the same rate and the concentrations of the substances stay the same.
• Le Chatelier's Principle

  • The equilibriums position can be changed by changing the reaction conditions:
  • Pressure
  • Concentration
  • Temperature
• What the equilibrium does?

  • When a change is made to a system, the position of the equilibrium moves to counteract the change that was made.
• Changing the temperature

  • If temperature is increased, the Equilibrium position moves in the direction of the endothermic process.
• Changing the pressure

  • If pressure increases in a reaction involving gases, the equilibrium position moves in the direction of fewest molecules of gas, to reduce pressure.