Kinetics
- Created by: emma
- Created on: 29-04-14 19:33
View mindmap
- Kinetics
- Activation energy
- The minimum amount of energy required for a reaction to take place
- For a reaction to take place
- Particles must collide with enough energy to overcome activation energy
- Must collide in the correct orientation
- Increase rate of reaction
- Increase temperature
- average energy of particles increases
- Particles move faster
- more particles have a collision energy greater than Ea
- Number of successful collisions per second increases
- more particles have a collision energy greater than Ea
- Particles move faster
- average energy of particles increases
- Decrease particle size
- Surface area increases
- Number of successful collisions per second increases
- Surface area increases
- Increase pressure
- Number of particles per unit volume increases
- Number of successful collisions per seecond increases
- Number of particles per unit volume increases
- Increase concentration
- Number of particles per unit volume increase
- Number of successful collisions per second increase
- Number of particles per unit volume increase
- Add a catalyst
- What
- substance which increases rate of chemical reaction with out itself being chemically changed
- How
- Substance which provides an alternative rout for the reaction with a lower activation energy
- What
- Increase temperature
- Maxwell boltzmann
- Area under curve is total number of particles
- Peak represents most probable energy (energy possessed by largest proportion of particles)
- Area under curve to right of Ea are particles with Ea
- Increase temp moves curve to the right and lower
- Activation energy
Comments
No comments have yet been made