Multiple Choice
Which values of the equilibrium constant K indicate that there is more product B than reactant A at equilibrium for the reaction A ⇌ B?
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16. Chemical Equilibrium
Equilibrium Constant K
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Given the reaction: FeCl_3(aq) + 3NH_4SCN(aq) ⇌ Fe(SCN)_3(aq) + 3NH_4Cl(aq), which of the following is the correct equilibrium constant expression (K) for this reaction?
A
K = [Fe(SCN)_3][NH_4Cl]^3 / [FeCl_3][NH_4SCN]^3
B
K = [Fe(SCN)_3] / [FeCl_3][NH_4SCN]^3
C
K = [FeCl_3][NH_4Cl]^3 / [Fe(SCN)_3][NH_4SCN]^3
D
K = [FeCl_3][NH_4SCN]^3 / [Fe(SCN)_3][NH_4Cl]^3
Verified step by step guidance1
Identify the balanced chemical equation: FeCl_3(aq) + 3NH_4SCN(aq) ⇌ Fe(SCN)_3(aq) + 3NH_4Cl(aq).
Recall that the equilibrium constant expression (K) is the ratio of the product of the concentrations of the products raised to their stoichiometric coefficients to the product of the concentrations of the reactants raised to their stoichiometric coefficients.
Write the general form of the equilibrium constant expression: \(K = \frac{[\text{products}]^{\text{coefficients}}}{[\text{reactants}]^{\text{coefficients}}}\).
Apply this to the given reaction: \(K = \frac{[Fe(SCN)_3][NH_4Cl]^3}{[FeCl_3][NH_4SCN]^3}\), where each concentration is raised to the power of its coefficient in the balanced equation.
Confirm that this expression matches the stoichiometry of the reaction and includes all aqueous species, excluding solids or pure liquids if any were present.
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