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activation energy
The minimum amount of energy that particles must collide with to react.
catalyst
Increases the rate of reaction by providing a different pathway for the reaction that has a lower activation energy.
They are not used up during the reaction.
collision theory
According to this theory, chemical reactions can occur only when reacting particles collide with each other and with sufficient energy.
effect of changing concentration on equilibrium
If increased, more products will be formed until equilibrium is reached again.
If decreased, more reactants will react until equilibrium is reached again.
effect of changing pressure on equilibrium
An increase causes the equilibrium position to shift towards the side with the smaller number of molecules.
A decrease causes the equilibrium position to shift towards the side with the larger number of molecules.
effect of changing temperature on equilibrium
If increased then the relative amount of products at equilibrium increases for an endothermic reaction and decreases for an exothermic reaction.
effect of concentration on reaction rate
Reacting particles will be closer together.
This means they will collide more often so there will be a higher rate of successful collisions and a faster rate of reaction.
effect of pressure on reaction rate
Reacting particles will be closer together.
This means they will collide more often so there will be a higher rate of successful collisions and a faster rate of reaction.
effect of surface area on reaction rate
There are more exposed reacting particles.
This means there are more frequent successful collisions so the rate of reaction increases.
effect of temperature on reaction rate
Particles will have more kinetic energy and so will move faster.
If the molecules are moving faster they will collide more often and, since they’ve gained kinetic energy, a larger proportion of the particles will have at least the activation energy.
For both these reasons the rate of reaction increases.
equilibrium
When a reversible reaction occurs in apparatus which prevents the escape of reactants and products, this is reached when the forward and reverse reactions occur at exactly the same rate.
Le Chatelier’s Principle
If a reaction at equilibrium is subjected to a change in concentration, temperature or pressure, the position of equilibrium will move to counteract the change.
rate of reaction
The measure of the amount of product formed or reactant used over time.
The units of rate of reaction may be given as g/s, cm3/s or mol/s.
reversible reaction
Reactions in which the products from the reaction can react together to form the original reactants. The direction of reversible reactions can be changed by changing the conditions.
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