unit 8 - reaction kinetics

rate of reaction

• change in the amount of susbtance with time

• rate = change in amount of reatants n products / time

collision theory

• particles must collide in the correct orientation with sufficent energy

• successful collisions take place if reactant particles have enough energy to react

non effective collisions

• Incorrect orientation 

• Not enough energy

• Particle bounce off each other preventing  chemical reaction

increasing collision theroy

• increased freuqeuncy of collisions

• more collisions per unit time

• number of particals with energy that is more than activational energy increases

effect of concentration, pressure, temperature on rate of reaction

• concentration increases, the rate of reaction increases

• pressure increases, the rate is faster

• temperature increases, rate increases

activational energy

the minimum energy that colliding particals must possess for successful collision to take place

catalyst

• subsatnce increases the rate of reaction but remains chemically unchnaged itself at the end of the reaction

• catalyst decreases the activational energy

• provides an alternate route for the reaction

• dont change the shape of a boltzmann distribution