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The principle basically says that chemical reactions will adjust to minimize the effect of any changes. When pressure increases by a decrease in volume, and there are more moles of gas on the reactant side, then the reaction will produce more products. When pressure increases by a decrease in volume, and there are more moles of gas on the product side, then the reaction will produce more reactants. This only applies to a pressure change that also changes the volume and concentration of the mixture, so a pressure change by adding gas like helium would have no effect on the reaction.
Le Chatelier's Principle is important because it explains why the questions about systems shifting in different directions are important. They are shifting either towards the reactants or towards the products in attempt to minimize the effect of external causes, such as increasing the pressure by decreasing volume. But, it's important to know that increasing the pressure by adding an inert gas does NOT cause the reaction to shift because concentrations aren't affected.
basically the reaction will "adjust" to keep K constant. if you add more products and throw off the equilibrium, the reaction will proceed to the left to form more reactants. Regarding the change in pressure, the reaction will proceed towards the side with less moles of gas; however, it is important to note that the change in pressure must result in a change in CONCENTRATION. if you add an inert gas, for example, you will still see a change in pressure, but it doesn't affect the concentration of the reactants or products.
Le Chatelier's Principle basically means that a reaction will adapt to any changes as a response to minimize the effect of the change. This means that if pressure is increased or decreased, Le Chatelier's principle tells us that the reaction will adjust to keep K, the equilibrium constant, stable.
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