1.5 - Kinetics Flashcards
1
Q
What must particles do in order to react?
A
Collide with sufficient energy (activation energy) and the correct orientation.
2
Q
Do most collisions result in a reaction?
A
No
3
Q
Define activation energy.
A
The minimum energy requied for a reaction to take place.
4
Q
What is the effect of increasing temperature on rate of reaction? Why?
A
- Increasng temperature increases the rate of reaction.
- Much higher proportion of particles have energy greater than the activations energy -> many more successful collisions per second -> increased rate.
5
Q
What is the effect of increasing concentration and pressure on the rate of reaction? Why?
A
- Increases concentration/pressure -> increased rate of reaction.
- There are more particles in a given volume -> more frequent successful collisions -> increased rate.
6
Q
What is a catalyst?
A
A substance which increases the rate of reaction but is not used up in the reaction.
7
Q
How do catalysts work and how do they increase the rate of reactions?
A
- Provide an alternative reaction pathway (one with lower activation energy).
- Lowers activation energy, so more frequent successful collisions, so increased rate.
