For a reaction in equilibrium, the species involved in the equilibrium constant expression are
gaseous and solid species
liquid and solid species
solid and dissolved species
gaseous and dissolved species
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In a chemical reaction at equilibrium, the forward and reverse reactions occur at the same rate, resulting in a dynamic balance where the concentrations of reactants and products remain constant over time. The equilibrium constant (K) expresses the ratio of the concentrations of products to reactants at equilibrium, raised to the power of their stoichiometric coefficients.
For a reaction involving gaseous and dissolved species, only these species contribute to the equilibrium constant expression because their concentrations directly affect the position of the equilibrium. Gaseous species are included because their concentrations can be easily controlled by changing pressure, while dissolved species are included because their concentrations can be controlled by changing the amounts of reactants or products dissolved in the solution.
Solid species, however, typically do not affect the equilibrium constant expression because their concentrations remain constant and do not change the position of equilibrium. Similarly, liquid species are usually omitted from the equilibrium constant expression for the same reason, unless they are reactants or products in a reaction involving significant changes in their concentrations.
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