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If there is a change in pressure caused by the volume to be halved, then the reaction will shift to the side of the equation with the smaller sum of coefficients. However, what exactly happens during that shift? For example, if it shifts towards the products, does that mean the concentration of products increases?
Yes, remember that Le Chatelier's principle wants equations to balance out any changes that might occur in the environment. This means that when pressure is increased, the side with the less amount of moles will be favored to try and balance it out. For example, if the products have the smaller amount of moles, more reactants will be turned into the product and therefore the concentration of the products will increase and the concentration of the reactants will decrease.
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