The gas phase reaction \(2\mathrm{NO_2(g)} \rightarrow \mathrm{N_2O_4(g)}\) is an exothermic reaction. The decomposition of \(\mathrm{N_2O_4}\), in equilibrium mixture of \(\mathrm{NO_2(g)}\) and \(\mathrm{N_2O_4(g)}\), can be increased by :
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- lowering the temperature.
- increasing the pressure.
- addition of an inert gas at constant volume.
- addition of an inert gas at constant pressure.
The Correct Option is D
Solution and Explanation
(1) Lowering temperature favours the exothermic forward reaction, so decomposition decreases.
(2) Increasing pressure favours fewer moles, i.e. \(\mathrm{N_2O_4}\), so decomposition decreases.
(3) Inert gas at constant volume does not change partial pressures or concentrations, so no shift.
(4) Inert gas at constant pressure increases the volume, which lowers the partial pressures, so the equilibrium shifts to the side with more moles, i.e. decomposition of \(\mathrm{N_2O_4}\) increases.
Answer: (4) addition of an inert gas at constant pressure.
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