simple collision theory Flashcards
1
Q
what is meant by the term ‘rate’?
A
the change of concentration or amount of product produced over time
2
Q
how do you calculate rate of reaction?
A
(reactants used / product made) / time
3
Q
what is collision theory?
A
particles must collide in the right direction and have the minimum amount of kinetic energy for a reaction to take place
4
Q
what is ‘activation energy’?
A
the minimum amount of energy required to break the bonds of the reactants
5
Q
describe the effect of concentration on rate of reaction?
A
- increased concentration
- particles are closer together
- more frequent successful collisions
- increased rate of reaction
6
Q
describe the effect of temperature on rate of reaction?
A
- increased temperature
- more molecules have more than the activation energy
- particles move around more
- more frequent successful collisions
- increased rate of reaction
7
Q
describe the effect of pressure on rate of reaction?
A
- increased pressure
- more particles per unit volume= packed closely together
- more frequent successful collisions
- increased rate of reaction
8
Q
describe the effect of surface area on rate of reaction?
A
- increase surface area
- increases the number of exposed reactant particles
- more frequent succsessful collisions
- rate of reaction increases
