1.05 Kinetics
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What must particles do in order to react ?
Collide with sufficient energy (Ea) and in the correct orientation.
Do most collisions result in a reaction ?
No
Define activation energy (Ea).
The minimum energy that particles must collide with for a reaction to occur.
Draw / describe a labelled Maxwell-Boltzmann. Label the average energy, activation energy and most probably energy. Draw / describe how it changes depending on temperature.
What is the effect of increasing the temperature on a reaction ?
• Increasing the temperature in increases the rate of reaction • This is because the frequency of successful collisions increases as a much higher portion of particles have sufficient energy.
What is the effect of increasing concentration / pressure on rate of reaction ? Why ?
• It results in a faster rate of reaction • This is because there are more particles in a given volume, which means there are more frequent successful collisions.
What is a catalyst ?
A substance which lowers the activation energy of a reaction whilst not being used as a reactant.
How do catalysts work and how do they increase rate of reaction ?
• Catalysts provide an alternative pathway for the reaction (one with a lower Ea) • The lower Ea means a higher portion of particles have sufficient energy to react, so successful collisions become more frequent, giving a higher rate.