###### Equilibrium Constants

An equilibrium constant gives a numerical representation of the position of an equilibrium. It is calculated in a **homogenous** system, this means one all substances are in the same **phase** for example liquid, or gas. Therefore we have different constants depending on this state.

### Concentration Constant: Kc

This is the equilibrium constant calculated using concentrations. It is calculated as follows.

The value of Kc only applies at a constant temperature. If you are a bit confused by mathematics then this is the expression in words. To calculate Kc you take the concentrations of the **products**, and then do each one to the power of the **number of moles** of it, from a balanced equation. Then do the same for the reactants, and divide products by reactants.

The **units of Kc** depend on how many moles there are on either side of the equation. You can do a quick calculation to work out what the units will be, for example...

If there were the same number of moles of both sides of the equilibrium, then the top and bottom would cancel, and there would be no units of Kc.

### Pressure Constant: K_{p}

This a way of getting the equilibrium constant when the system is a **gas**. In order to work this out, we first need to know the **partial pressures** of each molecule in the reaction.

Now that we have the partial pressures, it is now possible to calculate the value of K_{p}.

### Effects of Changing Conditions

If you have a look at the material on equilibria you will see that the position of equilibria varies according to how conditions are varied. **Le Chatelier's** principle states that a system will **oppose** a change. To predicting how the value will change you must remember that the closer to the left the equilibrium is, the smaller the value of K is.

Therefore increasing temperature shifts the eqilibrium in the **endothermic** direction.

Changing the **pressure** only affects gases, i.e. it only alters K_{p}. So increased pressure will move the equilibrium to the side with **fewer moles**.

What happens with **concentration** is a little more complicated, obviously this will only affect Kc and the key is that changing the concentration of one species will alter the concentrations of all other species so that the value of Kc remains the same. If the concentration of a **reactant** is increased the the equilibrium will move to the right to remove the product. Changes in concentration for Kc are equivalent to partial pressure changes in K_{p}.

The use of a catalyst has no affect on the equilibrium constant or the equilibrium (it increases the rate of reaction in both directions).