Kinetics
- Created by: Shannon
- Created on: 13-03-14 10:51
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- Kinetics
- Le Chateliers principle
- If a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.
- Affect of pressure
- Will shift equilibrium in the direction of the reaction with fewest particles
- Affect of temperature
- "heat favours the endothermic reaction"
- Will shift equilibrium to the endothermic reaction
- "heat favours the endothermic reaction"
- The collision theory
- Particles need to collide
- An increase in concentration
- There are more particles in the same amount of space.
- This means that particles are more likely to collide, increasing the frequency of collisions.
- There are more particles in the same amount of space.
- An increase in pressure
- The same number of particles are present but in a smaller space.
- This means that particles are more likely to collide, increasing the frequency of collisions.
- The same number of particles are present but in a smaller space.
- An increase in surface area
- Increases the area for particles to collide with.
- More collisions = faster rate of reaction
- Increases the area for particles to collide with.
- An increase in concentration
- Particles must have sufficient energy - possess the activation energy
- Addition of a catalyst
- Lowers the activation needed for the reaction to occur
- More particles have E > Ea
- Reaction occurs at a faster rate
- More particles have E > Ea
- Lowers the activation needed for the reaction to occur
- Addition of a catalyst
- Particles need to collide
- Factors affecting reaction rate
- Surface area
- Concentration
- Temperature
- Pressure
- Catalyst
- Maxwell-Boltzman distribution
- Particles do not all possess the same energy
- Energies are distributed
- Factors affecting distribution
- Catalyst
- Does not effect the average energy of the particles
- Activation energy is lowered
- More particles with E > Ea
- Activation energy is lowered
- Does not effect the average energy of the particles
- A decrease in concentration
- More particles have energy less than Ea
- Catalyst
- Particles do not all possess the same energy
- Activation energy
- The minimum amount of energy required for a chemical reaction to occur
- Catalyst
- A substance that speeds up the rate of reaction, by using an alternative pathway with lower activation energy.
- The substance is not used up during the reaction.
- A substance that speeds up the rate of reaction, by using an alternative pathway with lower activation energy.
- Le Chateliers principle
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