Why does temperature change the equilibrium constant of a reversible reaction?

Equilibria are governed by Le Chateliers principle:

When a stress is applied to a system in a dynamic equilibrium, that reaction is favored which partially counteracts the stress.

So if our reaction is exothermic, the forward reaction produces heat:

X + Y <--> Z + heat

If we increase the temperature, Le Chatelier's principle tells us that the reaction will respond by favoring the reverse reaction in order to consume heat and partially counteract the increase.

If we decrease the temperature, the forward reaction will be favored which will create heat and partially counteract the decrease.

In an endothermic reaction, the opposite is true.

The equilibrium constant is determined by the concentrations of the products. So when we increase or decrease the heat, products or reactants are consumed. This therefore alters the concentrations of the products and reactants and hence, the equilibrium constant.

This principle can also be applied to changes in pressure, and changes in the concentrations of the reactants and products. This allows us to determine how a reversible reaction will respond to changes and hence, the effect on the equilibrium constant.

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