kinetics Flashcards
Collision theory
5.1 Collision theory
For a reaction to take place between two particles, they must collide with enough energy to break the bonds and also the collision must be between the parts of the molecule that are going to react together
Activation energy
5.1 Collision theory
The minimum amount of energy the molecule must have for the reaction to start, the energy between the reactants and the transition state
why most collisions do not lead to a
reaction?
5.1 Collision theory
This is due to two main factors: the energy of the collision and the orientation of the colliding particles.
Maxwell-Boltzmann distribution
5.2 Maxwell–Boltzmann distribution
The distribution of energies of the molecules in a gas or liquid
why does the curve begin at (0,0) on Maxwell–Boltzmann distribution graphs ?
5.2 Maxwell–Boltzmann distribution
So no particles have 0 energy - which is why the curve must start from the origin.
- The origin is zero particles and zero energy
effect of Temperature increase
5.3 Effect of temperature on reaction rate
Increases the speed of the molecule, which increases both the speed of the molecules and the frequency of collisions
effect of Concentration increase
5.4 Effect of concentration and pressure
Increases the frequency of collisions between the molecules, which increases the rate of the reaction
effect of Pressure increase
5.4 Effect of concentration and pressure
Increases the frequency of collisions between the molecules, which increases the rate of the reaction
effect of Surface area increase
5.5 Catalysts
Increases the rate of reaction because there are more sites for reaction
Using a catalyst
5.5 Catalysts
Changes the rate of a reaction without chemically changing itself
Provide a different pathway for the reaction, one with a lower activation energy
