Kinetics and Equilibria
- Created by: leenaq
- Created on: 04-03-14 18:19
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- Kinetics and Equilibria
- Reaction Rates
- A reaction will not happen unless
- they collide in the right direction
- need to be facing each other the right way
- they collide with the least amount of kinetic energy
- activation energy
- the minimum energy required for particles to react
- the lower the activation energy, the easier the reaction happens
- activation energy
- they collide in the right direction
- Maxwell-Boltzmann distribution
- its is a theoretical model that explains scientific observations
- what it shows
- the speed of molecules ( the number of molecules against kinetic energy
- the molecules that have more than the activation energy are the ones that react
- variables that effect reaction rates
- increasing temperature
- the molecules will have more kinetic energy and will move faster
- increasing concentration(or pressure)
- means the particles are closer together
- increasing surface area
- a smaller particle size means that more particles can come in contact.
- using a catalyst
- they lower the activation energy hence more particles have enough energy to react
- increasing temperature
- catalysts
- increases the rate of a reaction by providing an alternative reaction pathway with a lower activation energy.
- a homogeneous catalyst is in the same state as the reactants.
- they speed up the reactions by forming one or more intermediate compounds with reactants
- A reaction will not happen unless
- chemical equilibria
- reversible reactions
- the reaction can go either direction
- the forward reaction slows down and the reverse reaction speeds up
- after a while the forward and reverse reactions are going to be the same
- dynamic equilibrium
- when the amounts of reactants and products won't be changing ( seems like nothing is happening )
- can only happen in a closed system
- changing concentration, pressure or temperature alters the position go equilibrium
- if the position of equilibrium moves left you get more reactants
- of the position of equilibrium moves right you get more products
- position of equilibria
- catalysts
- no effect on the position of equilibrium
- concentration
- when you increase the concentration of a reaction equilibrium tries to get rid of extra reactant, making more product and vice versa
- pressure
- increasing the pressure shifts equilibrium to the side where less gas molecules are. reduces pressure
- decreasing pressure shifts equilibrium to the side where more gas molecules are, raises pressure
- temperature
- increasing the temperature, equilibrium shifts in endothermic direction to absorb heat
- decreasing the temperature, equilibrium shifts in exothermic direction to replace heat
- catalysts
- reversible reactions
- Reaction Rates
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