The effect of concentration on a system in equilibrium

In the reaction:

N₂ + 3H₂ 2NH₃

If we increase the concentration of any of the species(i.e. add more of them in), the equation will tend to shift to the other side, so as to keep K_c constant.

For instance if we add more N₂ into the reaction, that makes the bottom line larger, and therefore the value for K_c would be smaller. However, Le Chatelier's Principle brings us to see that the equation 'moves' in the direction which would increase K_c, to bring it back to its 'constant' value. Therefore, adding N₂ will cause to equation to move to the right, causing more ammonia (NH₃) to be produced.

So adding more NH₃ will cause the equation to move to the left, and more N₂ and 3H₂ will be produced.

Site designed by Bryan Le Gear and Fintan Breen.