For the reaction 2N 2O (g) ⇌ O 2 (g) + 2N 2 (g), what happens to the equilibrium position if the pressure increases?

Equilibrium will shift in forward direction.

Explanation:

According to Le Chatelier's Principle, the change in any state of the equilibrium say temperature, volume, pressure, or the concentration, the equilibrium will oppose these changes and will shift in such a way that the effect cause must be nullified.

Effect of the change in the pressure:

If the pressure is increased, the equilibrium of the reaction is disturbed, so, the reaction will move in order to decrease the pressure.

The molecules of gas are responsible for the pressure and thus to nullify this effect or to decrease the pressure, the equilibrium will shift in a direction where there are less number of gaseous molecules.

For the reaction given,

2N₂O (g) ⇄ O₂ (g) + 2N₂ (g)

The number of gaseous molecules in the product (2) is less than the reactant (2 + 1), so the equilibrium will shift in forward direction.