1.5 Kinetics
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What must particles do in order to react?
Collide with sufficient energy (activation energy) and the correct orientation
Do most collisions result in a reaction?
no
Define Activation Energy.
The minimum energy that particles must collide with for a reaction to occur
What is the effect of increasing temperature on rate of reaction? why?
Increasing temperature → increased rate of reaction Much higher proportion of particles have energy greater than the activation energy → many more successful collisions per second →increased rate
What is the effect of increasing concentration/pressure on rate of reaction? why?
Increased concentration/pressure → increased rate of reaction There are more particles in a given volume → more frequent successful collisions → increased rate
What is a catalyst?
A substance which increases the rate of reaction but is not used up in the reaction
How do catalysts work and how do they increase the rate of reaction?
Provide an alternative reaction pathway (one with a lower activation energy) Lowers activation energy, so more particles have energy > activation energy, so more frequent successful collisions, so increased reaction rate