Le Chatelier's Principle when an inert gas is added

[Marcus Lagman 2A]

Hello!

I am going over and refreshing on chemical equilibrium for the upcoming final. When an inert gas is added, how does that affect the equilibrium? Are there certain conditions in which would cause a shift to the left or right? Does it relate to pressure/volume? If anyone can clarify, it would be appreciated!

[shevanti_kumar_1E]

If the pressure of the reaction vessel is increased by adding an inert gas there is no change to the equilibrium constant because the mol of reactant, mol of product, and volume are constant. Since there is no change in the concentration of the reactant and no change in the concentration of the product K doesn't change.

[Nika Gladkov 1A]

Addition of an inert gas does not affect equilibrium because it affects the partial pressures of the products and reactants equally. Therefore, it does not cause the reaction to shift either to the left or right. Addition of reactant or product to increase pressure would shift equilibrium. Also, lowering volume will cause the equilibrium to shift to the side with less moles of gas.

[Kayle Lim 2C]

Equilibrium is not affected or changed due to the addition of any inert gas. There is essentially no change to the production rates of reactants meaning there would be no favoring within the equation. Equilibrium would still hold with added pressure since the products and reactants do not change. With this, shifting does not occur and everything stays in equilibrium.

[edward_brodell_2I]

The same holds true in terms of concentration which is how Dr.Lavelle explained it in terms of the no effect of the inert gas added.