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Yes it does. Increasing the pressure of a reaction by decreasing volume favors the side of the reaction with less mols of gas. If you increase pressure by adding an inert gas, it doesn’t change the concentration of reactants or products.
If the change in pressure changed the volume, it affects the concentration. If the change in pressure was caused by the addition of an intert gas, the volume hasn't changed so the concentrations have not changed.
As an addition to the earlier replies: Although changing the pressure changes the concentration of the products and reactants, their ratio will return to the equilibrium constant, Kp. Only a change in temperature changes Kp, not the pressure or concentration of products and reactants.
When there is an increase in pressure, the equilibrium will shift towards the side of the reaction with fewer moles of gas. When there is a decrease in pressure, the equilibrium will shift towards the side of the reaction with more moles of gas.
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