Here are the essential concepts you must grasp in order to answer the question correctly.
Chemical Equilibrium
Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In the given reaction, H2 and I2 combine to form HI, and at equilibrium, the concentrations of all species remain unchanged over time. Understanding this concept is crucial for analyzing the provided equilibrium concentrations and calculating the equilibrium constant (Kc).
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Equilibrium Constant (Kc)
The equilibrium constant (Kc) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium, raised to the power of their stoichiometric coefficients. For the reaction H2(g) + I2(g) ⇌ 2 HI(g), Kc is calculated as [HI]^2 / ([H2][I2]). This constant provides insight into the position of equilibrium and how it shifts with changes in concentration or temperature.
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Le Chatelier's Principle
Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. This principle helps predict how changes in temperature, pressure, or concentration will affect the equilibrium position of the reaction. In the context of the question, understanding this principle is essential for interpreting how Kc values might vary with temperature.
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