Final answer:
Without knowing the equilibrium constant (K) for the reaction between Fe³⁺ and SCN⁻, it's not possible to calculate the equilibrium concentration of FeSCN²⁺. An ICE table method is commonly used for such a calculation when K is known.
Step-by-step explanation:
To determine the equilibrium concentration of FeSCN²⁺, we must first recognize that the reaction between Fe³⁺ and SCN⁻ to form FeSCN²⁺ is an equilibrium process and follows the law of mass action. However, the question does not provide the equilibrium constant for the reaction, which is required to calculate the equilibrium concentrations. Without this information or additional context such as whether one of the reactants is in excess or the assumption that the reaction goes to completion, it isn't possible to provide a specific numerical answer.
In real-life scenarios, if the equilibrium constant (K) were known, you could use the initial concentrations of the reactants and the stoichiometry of the balanced reaction to set up an ICE table (Initial, Change, Equilibrium) to solve for the equilibrium concentrations.
Since the exact equilibrium constant is not provided in the given data, we can't complete the ICE table and thus we cannot calculate the equilibrium concentration of FeSCN²⁺ in this case.