Kinetics
- Created by: Chloe Trotter
- Created on: 13-04-16 11:34
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- Kinetics
- Collision theory
- Reactions can only occur when collisions take place
- Particles must have the required energy for a reaction to take place when they collide
- Activation energy- minimum energy needed for particles to collide sucessfully
- To break the bonds
- Maxwell Boltzmann distribution
- Shows the spread of energies that molecules have at a particular temperature
- Area under the curve represents the number of particles
- Starts at 0 because no molecules have no energy
- A few particles have low energy because collisions can slow them down.
- Most probable energy is the peak
- Emp
- Not the mean energy
- To the right of the Emp
- Never meets the x axis because there is no maximum energy for molecules
- Shows the spread of energies that molecules have at a particular temperature
- Increasing the temperature
- As the temperature increases the particles have more energy
- Collide more frequently
- More particles collide with the required activation energy
- Distribution shifts to the right in the MBD graph
- Emp and mean energy both shift right
- Total area under the curve remains the same
- Same number of particles
- Wider range of energies than lower temperatures
- Bigger proportion of particles than the activation energy
- Frequency of successful collisions increases
- Bigger proportion of particles than the activation energy
- As the temperature increases the particles have more energy
- Increasing the concentration/pressure
- More particles per unit volume
- Particles collide more frequently
- Higher frequency of successful collisions
- Doubling concentration/rate would mean double the number of particles per unit volume
- Peak (Emp) stays at the same point but the curve is higher
- Greater area under curve because there is more particles
- More particles per unit volume
- Adding a catalyst
- Increases the rate of reaction by offering an alternative route with a lower activation energy
- Activation energy is lower so more particles will have that energy
- Higher frequency of sucessful collisions
- Activation energy
- Increasing surface area
- Causes collisions to occur more frequently
- Incrases the rate of reactions
- Make it smaller
- Collision theory
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