Unit 3 OAS2

• • Two main aspects that determine if successful are:

     1. Collisions must have sufficient energy.

     2. Collisions must occur in a correct orientation.
• • Increase temperature will increase the average kinetic energy of particles, increase the frequency of collisions, increase proportion of particle with sufficient energy to react. Therefore, increase reaction rate
• Higher surface area will more ‘stuff’ to bump into, increase the frequency of collisions, thus higher reaction rate.
• • Increase catalyst will create alternative reaction pathway, low activation energy, and increase the proportion of successful collisions. Therefore, higher reaction rate.
• Compare Extension Reaction and Rate of Reaction

  • Extension Reaction: Indicates the amount of product formed when the system reaches equilibrium. 

  Rate Reaction: Measure of [Reactants] and [Products] over a period of time.
• Q  > Kc, a net reverse reaction is occurring to regain/reach equilibrium.
• • Q < Kc, a net forward reaction is occurring to reach equilibrium. 
• Le Chatelier’s Principles :

  ‘If a change is applied to an equilibrium system, the equilibrium will shift to partially oppose the effects of that change.’