Final answer:
Increasing the pressure in a chemical reaction causes the equilibrium to shift towards the side with fewer moles of gas molecules.
Step-by-step explanation:
Increasing the pressure in a chemical reaction will result in the shift of the equilibrium to the side with fewer moles of gas molecules. This is known as Le Chatelier's principle, which states that a system at equilibrium will respond to a stress by moving in a direction that reduces the stress.
For example, let's consider the reaction N2(g) + 3H2(g) <-> 2NH3(g). If the pressure is increased, the equilibrium will shift towards the side with fewer moles of gas molecules, which in this case is the reactant side. As a result, more N2 and H2 will react to produce more NH3 to alleviate the increase in pressure.
In summary, increasing the pressure in a chemical reaction will cause the equilibrium to shift towards the side with fewer moles of gas molecules.
Learn more about Chemical Equilibrium