What happens to the equilibrium position if the pressure is increased in a gaseous reaction?

When the pressure in a gaseous reaction is increased, the equilibrium position shifts in response to reduce that pressure. According to Le Chatelier's principle, a system at equilibrium will adjust to counteract any changes imposed on it. In the case of increasing pressure, the system will shift in the direction that produces fewer moles of gas.

This is because reducing the number of gas molecules results in a lower pressure, thereby counteracting the initial increase. Therefore, if one side of the equilibrium has more moles of gas than the other, the system will favor the side with fewer moles of gas upon the increase of pressure. This phenomenon is essential for understanding how reactions behave under different conditions and is a fundamental concept in the study of chemical equilibria.