What are the factors that affect the rate of a chemical reaction?

For a reaction to occur molecules must collide with energy greater than or equal to the activation energy, in the correct orientation. The factors affecting the rate of a reaction are:
Pressure of reacting gases- more molecules in a given volume of gas means more collisions in a given time therefore more successful collisions in a given time and a faster rate of reaction.
Concentrations of reactants in solution- more molecules in a given volume of solution means more collisions in a given time therefore more successful collisions in a given time and a faster rate of reaction.
Surface area of solid reactants- the greater the surface area of the solid, the more molecules that are available to react at a given time, therefore more frequent successful collision and a faster rate of reaction.
Temperature- the greater the temperature the greater proportion of molecules have energy greater than or equal to the activation energy and therefore a greater proportion of collisions are successful. The molecules also have more kinetic energy so move more quickly and therefore collisions are more frequent and therefore there are more successful collisions in a given time and the rate of reaction increases.
Catalysts- a catalyst speeds up the rate of reaction without being used up in the reaction itself. It does this by providing an alternate reaction pathway with a lower activation energy.