Kinetics
Rate of Reaction:
The change in concentration of a reactant/product in a certain period of time (mol dm-3 s-1).
A reaction will go faster if:
• There are more collisions per second
… and/or…
• A greater frequency of particles have sufficient
energy.
Activation Energy (Ea): The minimum energy required
for a successful collision
Factors Increasing the Speed of a Reaction
• Increase Concentration (Liquid) / Pressure (Gas)
o More particles in a given volume.
o More frequent collisions.
• Increase Surface Area
o Greater number of exposed particles which can be involved in a collision.
o More frequent collisions.
• Increase Temperature:
o Particles have more kinetic energy.
o More frequent collisions.
o Number of particles with E ≥ Ea increases.
o Frequency of successful collisions increases.
• Use of a Catalyst:
o Provides an alternate reaction pathway with lower Ea.
o Number of particles with E ≥ Ea increases.
o Frequency of successful collisions increases.
Rate of Reaction:
The change in concentration of a reactant/product in a certain period of time (mol dm-3 s-1).
A reaction will go faster if:
• There are more collisions per second
… and/or…
• A greater frequency of particles have sufficient
energy.
Activation Energy (Ea): The minimum energy required
for a successful collision
Factors Increasing the Speed of a Reaction
• Increase Concentration (Liquid) / Pressure (Gas)
o More particles in a given volume.
o More frequent collisions.
• Increase Surface Area
o Greater number of exposed particles which can be involved in a collision.
o More frequent collisions.
• Increase Temperature:
o Particles have more kinetic energy.
o More frequent collisions.
o Number of particles with E ≥ Ea increases.
o Frequency of successful collisions increases.
• Use of a Catalyst:
o Provides an alternate reaction pathway with lower Ea.
o Number of particles with E ≥ Ea increases.
o Frequency of successful collisions increases.
