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Inert Gases have no effect on the equilibrium reaction because they do not interact with either the reactants and products undergoing equilibrium. They do not interact with them because noble gases are extremely stable.
As stated already, inert gases are exempt as they are stable and seldom interact with species involved in reactions. You can think of them as "pure" substances like liquids and solids which are also exempt from the equilibrium constant.
In the video modules he explained that inert gasses do not affect the reaction because they do not change the concentration of products or reactants. When pressure increases by decreasing volume, the concentration increases, so the reaction is affected, but adding inert gasses does not increase or decrease the concentration.
Pressure change only affects a reaction if it is changing the concentration. Which is why when we change the volume the moles stay constant, but we effectively change the concentration or molarity. The concentration in turn affects the reaction. When we introduce an inert gas it is extremely stable and does not reactant. It does not create products or reactants so the concentrations do not change.
Increasing pressure by inserting an inert gas will not change the way the reaction leans. Only increasing pressure by reducing volume will affect the reactant quotient which will change the direction that the reaction favors.
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