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His principle states a change in pressure, temperature, or concentration of a reactant when applied to a system, the system will counteract the change and shift accordingly in order to return back to equilibrium.
It basically states that if a system in equilibrium is disturbed in some way, the system will shift to counteract the change and return to equilibrium. Dr. Lavelle’s main example for Friday’s lecture involved adding/removing product/reactants. For example, if you were to add more reactant, Le Chatlier’s principle tells you that the system will make more product in order to shift back to equilibrium. The principle is also used in regards to pressure and temperature.
It's a principle that explains how a reaction adjusts and minimizes the effect of change brought by circumstances that disrupts its equilibrium state. The affecting conditions can be change in molar concentration, pressure or temperature. For instance, an increase in the molar concentration of products will shift the reaction to the left to yield more reactants. The same concept applies when there are more reactants, moving the reaction to the right.
The General Idea of Le Chatelier's principle is that a given system will respond to changes in the system so as to minimize the effects of said change. This entails a number of different characteristic responses to different types of changes in the system (Temperature, Volume, Concentration, etc.). For example, a reaction will shift in response to an increased concentration of reactants by favoring the production of the products in order to reach the same desired ratio of Products to reactants in order to reestablish equilibrium.
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