Kinetics Flashcards
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 ROR
Much higher proportion of particles have energy greater than the activation energy→more successful collisions per second→increased rate
What is the effect of
increasing concentration/pressure on ROR? why?
Increased concentration/pressure → increased ROR
There are more particles in a given volume → more frequent successful collisions → increased rate
What is a catalyst?
A substance which increases the ROR but is not used up in the reaction
How do catalysts work and how do they increase the ROR?
Provide an alternative reaction pathway with a lower activation energy
Lowers activation energy, so more particles have energy >activation energy, so more frequent successful collisions, so increased ROR
