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The easy way to tell what changes will occur is to see how the moles of gas on the reactants and products sides differ. If the volume (moles of gas) is lower on the products side, then the reaction shifts to the right but if the volume (moles of gas) is higher on the products side, the reaction shifts left. Essentially changes in pressure indicate changes in volume, which indicates changes in concentration so the reaction shifts directions. But K won't change because the temperature is still the same.
When it comes to the partial pressure of a reactant/product changing, you can basically think of it as a change in concentration. So if the partial pressure of a reactant increased, then the reaction would shift to the right/to the products. But if they're talking about the pressure of the reaction overall, that's when you consider the moles of gas to determine what will happen.
Look at which side is affected more in terms of the exponents when you solve for a new Q. When volume is halved, concentration doubles and then apply the exponents to that double to find if Q is greater then or less than K, then decide which direction the reaction will proceed in.
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