6.2.1 –Describe the kinetic theory in terms of the movement of particles whose average energy is proportional to temperature in kelvins
The average energy calculated using each particle is proportional to the temperature in Kelvin. Particles move randomly in a substance as they contain kinetic energy. For example, increasing the temperature is would increase the average kinetic energy, so the particles have more energy. However at 0 Kelvin (absolute zero/-273°C) particles do not have kinetic energy at all.
6.2.2 –Define the term activation energy Ea
Definition of activation energy Ea | The minimum value of kinetic energy which particles must have before they are able to react |
6.2.3 –Describe the collision theory
Three factors that affect the rate of reaction
1. Collision frequency: | If the frequency of collision is higher, it is more likely that the probability of collision would be more successful. |
2. Number of particle with E≥Ea: | If the particles need to overcome repulsion between molecules or to break bonds in the reactants, they must have a minimum amount of energy, in order for collision to take place. For a successful reaction, the kinetic energy value of the particles must be greater than the activation energy [E ≥ Ea] will successfully collide. |
3. Appropriate collision geometry or orientation: | Particles must have the right collision geometry in order for the collision to be successful, so the reaction takes place. |
