How does removing a product shift the equilibrium?

Removing a product shifts the equilibrium towards the products side, increasing the rate of the forward reaction.

In a chemical reaction, equilibrium is the state where the concentrations of the reactants and products remain constant over time. This doesn't mean that the reaction has stopped, but rather that the forward and reverse reactions are happening at the same rate. This concept is described by Le Chatelier's Principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.

When a product is removed from the system, the equilibrium is disturbed. According to Le Chatelier's Principle, the system will respond by trying to replace the removed product. This is achieved by shifting the equilibrium position to the right, towards the products side. This increases the rate of the forward reaction, producing more of the product to compensate for the loss.

For example, consider the reversible reaction where nitrogen and hydrogen react to form ammonia:

N2(g) + 3H2(g) ⇌ 2NH3(g)

If some of the ammonia (NH3) is removed from the system, the equilibrium will shift to the right to produce more ammonia. This means that more nitrogen and hydrogen will react, increasing the rate of the forward reaction.

This concept is important in industrial processes where continuous production is required. By continuously removing a product, the reaction can be kept going in the desired direction, maximising the yield of the product. For instance, in the Haber process for the production of ammonia, the formed ammonia is continuously removed by cooling and liquefaction, driving the reaction to the right and increasing the yield of ammonia.