1.5 Kinetics Flashcards
(8 cards)
1
Q
KEY DEFINITION: Activation energy
A
The minimum energy required to start a reaction by the breaking of bonds
2
Q
KEY DEFINITION: rate of reaction
A
The change in concentration of a substance in a given time
3
Q
Why do most collisions do not lead to a reaction?
A
- the particles don’t have the activation energy
- the particles are in the wrong orientation
4
Q
How does increasing concentration affect the rate of reaction?
A
- increases the rate of reaction
- there are more particles in a given volume
- more frequent successful collisions
5
Q
How does increasing pressure affect the rate of reaction?
A
- increases the rate of reaction
- more particles in a given volume
- more frequent successful collisions
6
Q
How does increasing surface area affect the rate of reaction?
A
- increases the rate of reaction
- more points of contact with the other reactant
- more SA is available for collisions
- more frequent successful collisions
7
Q
How does increasing temperature affect the rate of reaction?
A
- increases the rate of reaction
- particles gain more energy so a greater proportion of particles have the Ea
- more frequent successful collisions
8
Q
How do catalysts affect the rate of reaction?
A
- provides an alternative reaction pathway with a lower Ea
- more particles have the Ea
- more frequent successful collisions
