Kinetics

• collision theory


  • for a chemical reaction to take place, particles need to collide with sufficient energy
• Maxwell-Boltzmann distribution curve:

  (Area under curve represents total number of molecules)

  
• Why does the curve start at the origin?


  No particles have zero energy
• Effect of concentration/pressure on rate of reaction


  • concentration: there’s more molecules in the same area, increasing the chance of successful collisions

  • pressure: same amount of molecules in less space, increases chance of collisions

  • Maxwell-Boltzmann curve shifts right
• Effects of catalysts on rate of reaction 


  • increases rate of reaction without being used up

  • provides an alternative pathway with a lower activation energy

  • Maxwell-Boltzmann curve doesn't change shape but activation energy moves left.