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Just to add on, it's because the concentrations of all the reactants and products increase proportionally when you change the volume if there is an equal number of moles on both side, so the equilibrium stays the same.
Minimizing the effect of changing volume is dependent on what side has more moles, so if both sides are the same then there's no shift that will minimize the effect. Aka it doesn't shift left or right
To understand why by changing the volume, if the number of moles is different between reactants and products thus shifting the reaction left or right, you have to understand that volume and pressure are inversely related. You increase the volume, the pressure will decrease. So, in this circumstance, this change in volume will favor the side with more moles, bc the reaction will want to compensate for the loss in pressure by creating more moles of gas. On the other hand, if you decrease the volume, the pressure will increase, so the rxn will favor the side with less moles bc the rxn will want to compensate for the increase in pressure by making less moles.
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