Kinetics Flashcards
1
Q
State what is meant by the term activation energy
A
the minimum amount of energy required for a reaction to occur
2
Q
Explain the collision theory
A
in a reaction, two things can happen
- nothing
- the particles could collide causing a reaction
3
Q
what happens to the rate of reaction when you increase the temperature
A
- the particles have more energy which means they collide more frequently (minor factor)
- more particles have greater energy than the activation energy
4
Q
what happens to the rate of reaction when you increase concentration or pressure
A
more particles per unit volume so there is more of a chance that the particles will have frequent successful collisions
5
Q
Define what a catalyst is
A
it lowers the activation energy by providing an alternative pathway for a reaction
6
Q
What happens to the rate of reaction when you add a catalyst
A
It increases because more particles have enough energy to collide
