3.1.5. Kinetics

for a successful reaction to occur - collision between particles must have… - energy greater than activation energy - correct particle orientation (steric effect)

graph showing energy distribution of molecules

the most probable energy of the particles - will cause ineffective collisions as they dont have enough energy

nothing - represents total no of molecules = must remain constant

shifts to right (greater prop of molecules have energy greater or equal to activation energy) - increases KE of molecules - move faster = more frequent collisions + more frequent SUCCESSFUL collisions due to higher energy - increases rate of reaction

more molecules in same volume/same no of molecules in smaller volume = packed closer together ^collision bt molecules = more frequent + successful collision more likely = rate of rx increases

substance that increases rate of rx w/out being used up - provides alternative reaction path with lower activation energy

homogenous heterogenous

catalyst is in the same phase as the reactants e.g. all in solution

catalyst is in a different phase to the reactants e.g. reactants are gases but the catalyst used is a solid

lower Ea = greater proportion of molecule have the activation energy, and therefore have sufficient energy for an effective collision

shape unchanged - position of Ea shifts to left (greater prop of molecules have sufficient energy to react)