reactions, particles and collisions ยง
- particles colliding with a certain amount of energy cause reactions.
- activation energy : minimum amount of energy needed for reactions.
- rate of reactions dependency:
- frequency of collisions
- energy with which particles collide
- if particles collide with less energy than activation energy, will not pull. particles will just bounce off each other if energy lower than activation energy
- rate of reaction factors
- temperature
- concentration of dissolved reactants
- pressure of gaseous reactants
- surface area of solid reactants
- use of a catalyst
- โ
more โ
higher frequency
- reactions not steady rate. start off certain speed, and get slower until they stop.
- concentration of reactants decreases during reaction progress.
- reduces the frequency of collisions between particles and reaction slows down.
- the effect of increasing temperature on the rate of reaction:
- increased average kinetic energy of particles
- increased velocity/speed of particles
- increased frequency of collisions
- increased proportion of collisions with sufficient kinetic energy to overcome activation energy
- increased frequency of *successful collisions; increased rate of reaction