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When pressure is increased by decreasing the volume, equilibrium shifts to to the side with less moles of gas because the concentrations of each compound is being increased according to the equation P=n/v. If pressure is increased by decreasing the volume, then the concentration increases since v is a smaller number. Therefore, equilibrium will shift to the side with less moles of gas.
I remembered that when the pressure was increased it moved to the side with fewer moles because if there is more pressure, the gas wants more area to spread out. If there are fewer moles with more pressure the moles of gas are not as cramped.
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