Kinetics Flashcards
1
Q
define activation energy
A
Minimum amount of energy required for a reaction to occur
2
Q
what must happen for a reaction to occur
A
- particles must collide w E>Ea
3
Q
Why might a reaction occur very slowly?
A
- A small number of particles have E≥Ea
4
Q
If a reaction occurs very slowly because only a small number of particles have E≥Ea, why will all of the reactants eventually gain enough energy to react?
A
- Molecules gain energy
- Due to collisions
5
Q
Why do some particles only have a very small amount of energy?
A
- Collisions
- Cause some molecules to slow down or lose energy
6
Q
What is the rate of reaction?
A
- rate of change in concentration / per unit of time
7
Q
affect of temperature increase on rate
A
- More particles have E≥Ea
- Increases frequency of successful collisions
8
Q
affect of concentration increase on rate
A
- Increase in number of particles per unit volume
- Increases frequency of successful collisions
9
Q
affect of pressure increase on rate
A
- Increase in number of particles per unit volume
- Increases frequency of successful collisions
10
Q
When drawing the curve for a higher temperature:
A
- The High T peak must be further to the right
- The curves must only cross once
- High T curve is wider/broader
- The size of the shaded area is larger for High T
