Question

The gas phase reaction \[\ce{2NO2_{(g)} ⇌ N2O4_{(g)}}\] is an exothermic reaction. The decomposition of N₂O₄, in equilibrium mixture of \[\ce{NO2_{(g)}}\] and \[\ce{N2O4_{(g)}}\], can be increased by:

Options

• lowering the temperature

• increasing the pressure

• addition of an inert gas at constant volume

• addition of an inert gas at constant pressure

Answer 1

addition of an inert gas at constant pressure

Explanation:

Lowering the temperature will encourage the creation of \[\ce{N2O4_{(g)}}\] because the process is exothermic. Increasing pressure will encourage the creation of \[\ce{N2O4_{(g)}}\] as the amount of gaseous species in the atmosphere decreases.

The addition of an inert gas will have no impact on the equilibrium at constant volume. When an inert gas is supplied, the equilibrium will change under constant pressure in a way that leads to an increase in the number of moles of gaseous species. Therefore, the breakdown of \[\ce{N2O4_{(g)}}\] can be boosted by the injection of an inert gas.