Question

According to Le Châtelier's principle, how will an increase in pressure affect a gaseous equilibrium system?

Shift it toward the products
Shift it toward the reactants
Shift it toward the side with higher total mole concentration
Shift it toward the side with lower total mole concentration

Answer 1

Shift it toward the side with lower total mole concentration

Step-by-step explanation:

Le Châtelier's principle states that if there is a change in conditions (for example pressure, temperature) to a closed system in dynamic equilibrium, the equilibrium will shift to minimise the change.

Pressure is caused by the collision of gas molecules. The more molecules there are, the greater the pressure so the system must reduce in pressure to counteract the increase in pressure and restore equilibrium. It does this by shifting to the side with lower total mole concentration to decrease the pressure again.