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This principle states that if a side of a equation increases in concentration, then the reaction will shift toward the other direction. For example, if the concentration of the reactions is increased, the forward reaction will be favored to produce more product to maintain equilibrium. Likewise, if the reactants were decreased in concentration, then the reverse reaction will be favored in order to produce more reactants to maintain equilibrium.
Le Chatelier's Principle is the idea that "chemical reactions adjust to minimize the effect of any changes". Some effects that can cause changes includes adding/removing a substance of the reaction, changing pressure, and changing the temperature. Le Chatelier's Principle shows that when these changes occur, the reaction will react to this external change by becoming more product/reactant-favored to maintain equilibrium.
For example, if you have a reaction and you want there to be more product to be made you can cause this to happen by removing some of the product, the reactions wants to be as stable as possible and it does so by creating more product to reach this sort of equilibrium state. As mentioned in lecture, This is how many companies in the industry create more product.
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