Collision Theory Flashcards
1
Q
what needs to happen for a chemical reaction to take place?
A
the reactant particles need to collide with enough energy
2
Q
what is activation energy?
A
the amount of energy the particles need to react
3
Q
what does the overall rate of a reaction involving millions of particles depend on?
A
- collision frequency - how often do the particles collide with each other
- percentage success - what percentage of the collision have enough energy
4
Q
what are the four common factors that affect the rate of a reaction?
A
- solid surface area
- solution concentration
- temperature
- catalysts
5
Q
what is the equation for rate of reaction?
A
rate = collision frequency x percentage success
6
Q
why does higher solid surface area increase rate?
A
- more of the solid is exposed to the other particles
- so the collision frequency is higher
- so there are more successful collisions
7
Q
why does higher solution concentration/gas pressure increase rate?
A
- there are more particles per unit volume
- so the collision frequency is higher
- so there are more successful collisions per unit time
8
Q
why do higher temperature increase rate?
A
- the particles have more kinetic energy
- so the percentage of collisions with enough energy is higher
- so there are more successful collisions per unit time
9
Q
why do catalysts increase rate?
A
- they provide an alternative route with a lower activation energy
- so the percentage of collisions with enough energy is higher
- so there are more successful collisions per unit time
