Not all chemical reactions go to completion, most go backwards and forwards around a point somewhere in the middle, eventually coming to a stop. Of course, the reaction doesn’t cease at this point, the reaction continues to hover around the equilibrium point, which is why it is known as dynamic equilibrium.
Technically, equilibrium is defined as the point at which the rates of the forward and reverse reactions are equal.
We express the point of equilibrium using the equilibrium expression:
for the reaction aA + bB ⇄ cC + dD. K is the equilibrium constant, the larger it is, the more the reaction favours the products. Obtaining the equilibrium constant is simply a matter of substituting the equilibrium concentrations into the equilibrium constant.
Alternatively, you may be given K and the initial concentrations and asked to find the equilibrium concentration. There is an example here,
because I can’t get the example to format here. The procedure to answer these problems is as follow:
- Set up a table of concentrations showing the initial, change and final concentrations for all products and reactants.
- Substitute the “equilibrium concentrations” (including the x) into your equilibrium expression.