Basically, I know that equilibrium is when the amount of reactants and products you have in a solution remains the same and that it's connected to the rate of the forward and reverse reactions etc. However, I'm having trouble remembering the effects that changes in pressure or temperature have on an equilibrium apart from that the equilibrium shifts. I'm also a bit confused over how the amounts of reactants/products can remain the same, if successful collisions between molecules occur randomly; surely there must be random changes in how much of each you have? Or am I completely missing something?
Any help from any chemical manipulating wizards would be really, really appreciated
