When I learn the chemical equilibrium, I have a question that has confused me for long time. When I add inert gas into an equilibrium system,
(1) if it is under constant temperature and constant volume, I know that the equilibrium does not shift, since the molarity of each of the original part does not change.
(2) if it is under constant temperature and constant pressure, I am told that the equilibrium will shift towards the direction with more molecules. But why is that? Could anyone give me an explanation with deduction from equilibrium constant or Dalton's law of partial pressures or any other related concepts?
Thank you all.