For the electrochemical cell, Fe(s) | Fe²⁺(aq) || Cu²⁺(aq) | Cu⁺(aq) | Pt(s), determine the equilibrium constant (K_eq) at 25^$\circ$C for the reaction that occurs.

Question

Quizplus · Accepted Answer

The equilibrium constant (K) for a reaction can be determined from the standard cell potential (E°) using the Nernst equation or its derived formula, K = 10^(nE°/0.0591), where n is the number of moles of electrons transferred in the reaction. Without the specific E° value or the half-reactions provided, we cannot calculate K directly here. However, the correct choice is based on standard electrochemical series and the knowledge that a higher E° value corresponds to a larger K value, indicating a more spontaneous reaction. Given the setup, it implies a reaction where Fe is oxidized and Cu is reduced, typically resulting in a large K value due to the cell potential difference between Fe and Cu in the electrochemical series.

For the Electrochemical Cell, Fe(s) | Fe2+(aq) || Cu2+(aq) | ∘\circ∘

For the Electrochemical Cell, Fe(s) | Fe²⁺(aq) || Cu²⁺(aq) | $\circ$