At standard temperature and pressure, the reaction indicated...

At standard temperature and pressure, the reaction indicated by the following equation has an equilibrium constant, $K_{\mathrm{c}}$, equal to 0.021 . $$2 \mathrm{HI}(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g})$$ Calculate the equilibrium constant, $K_{\mathrm{c}}$, for the reverse equation.

At standard temperature and pressure, the reaction indicated by the following equation has an equilibrium constant, $K_{\mathrm{c}}$, equal to 0.021 .
$$2 \mathrm{HI}(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g})$$
Calculate the equilibrium constant, $K_{\mathrm{c}}$, for the reverse equation.

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Key Concepts

Chemical Equilibrium

Chemical equilibrium refers to the state of a reversible reaction where the rate of the forward reaction equals the rate of the reverse reaction, meaning the concentrations of reactants and products remain constant over time. This concept is fundamental in understanding how reactions reach a dynamic balance, and how changes in conditions can shift the equilibrium position according to Le Chatelier's principle.

Equilibrium Constant (Kc)

The equilibrium constant, represented as Kc for reactions in solution or gaseous systems, quantifies the ratio of product concentrations to reactant concentrations at equilibrium, each raised to the power of their respective coefficients in the balanced chemical equation. It is a measure of the extent to which a reaction proceeds and provides insight into the relative stability of the products versus the reactants under specific conditions.

Reversing Reactions and Reciprocal Relationship

When a chemical reaction is reversed, the new equilibrium constant becomes the reciprocal of the original equilibrium constant. This is because the roles of reactants and products are interchanged in the equilibrium constant expression, leading to an inversion of the ratio. This principle is essential for understanding how equilibrium constants are affected by changes in the direction of the reaction.

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