Final answer:
Le Châtelier's principle explains that a chemical equilibrium will shift to counteract changes in the concentration of reactants or products. An increase in reactants favors the forward reaction, while an increase in products favors the reverse reaction. The equilibrium constant (Keq) remains unchanged despite the shift in equilibrium position.
Step-by-step explanation:
Le Châtelier's Principle and Changes in Concentration
Le Châtelier's principle describes how a chemical equilibrium reacts to disturbances or stresses. Specifically, when the concentration of reactants or products in an equilibrium system changes, the system shifts in a way that counteracts this change. If the concentration of a reactant is increased, the system will respond by favoring the forward reaction to produce more products, thus reducing the concentration of the added reactant. Conversely, if the concentration of a product is increased, the system will favor the reverse reaction to consume the excess product. It's important to note that the equilibrium constant (Keq) does not change with alterations in concentration; it is only the equilibrium position that shifts.
This principle is fundamental in understanding how chemical reactions adjust to maintain balance when subjected to external changes in concentration. The system's response is an attempt to maintain the established ratio of products and reactants as described by the Keq, which is exclusive to a given reaction at a given temperature.
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