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One example Lavelle gave in class was adding Helium to a reaction. Since Helium is a noble gas, it is basically unreactive and will not affect the reaction/shift equilibrium. I don't think we have to understand exactly how Helium will just "sit" in the reaction, but the main idea is that noble gases are unreactive and adding them will not shift equilibrium.
Yeah so ideal gases like Helium and nitrogen, if the reaction vessel had none of them ideal gas within the reactants or products of the reaction, then ultimately the concentrations of them do not change. We learned the quick way that if volume is decreased (pressure increased) then equilibrium would shift to the side with "less molecules," but that only works due to the underlying concept of increased concentrations. So if an ideal gas is added but does not affect concentration, it can still be added to a vessel to increase overall pressure but will not affect equilibrium.
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