What happens to equilibrium when pressure is increased?

Hint: Le Chatelier's principle can be used to forecast the creation of reactants and products in an equilibrium process. Boiling point and pressure are inversely proportional. By applying the Le Chatelier principle, we can provide the answer to this query.

Complete Step by Step Solution:
Le-Chatelier’s Principle: If a chemical system is disrupted while it is in equilibrium, the system would respond in a way that counteracted the stress and disruption.

Let us understand this by an example as follows:
\[CO(g) + {H_2}O(l) \rightleftharpoons C{O_2}(g) + {H_2}(g)\]

The equilibrium of the reaction shifted to the right as the reactant concentration was raised.
The equilibrium of the reaction shifted to the left if the reactant concentration was reduced.

According to Le Chatelier's principle, if we increase the pressure, the equilibrium will shift, causing the pressure to drop once more. Pressure is created by the collision of the gas molecules with the container's surfaces. If there are more gaseous molecules present, the pressure will be higher.

When it comes to pressure changes, an increase in gaseous pressure would cause the equilibrium to shift in favour of the side with fewer molecules of the gas. If the pressure is reduced, the equilibrium will move in a direction that has more gaseous molecules.
According to Le Chatelier's principle, the equilibrium moves to the side with the lower number of gas molecules when the pressure is increased.

Note: We must be aware of a few elements that influence the change in equilibrium, including,
Changes in concentration:
Effect of change in temperature on equilibrium
Effect of catalysts on equilibrium
For example: When the concentration of hydrogen chloride is raised, the direction of the equilibrium change must be stated.

The given reaction is,
\[{H_2}(g) + C{l_2}(g) \rightleftharpoons 2HCl(g)\]
Le Chatelier's principle states that as hydrogen chloride concentration rises, the equilibrium moves to the left, producing more reactants.