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

Question

Quizplus · Accepted Answer

The equilibrium constant can be determined using the Nernst equation and standard electrode potentials. The reaction involves the reduction of Cu²⁺ to Cu⁺ and the oxidation of Fe to Fe²⁺. Calculating the standard cell potential and using the relation between cell potential and equilibrium constant, K_eq is found to be 8.6 x 10¹⁹.

For the Electrochemical Cell, Fe(s)| Fe2+(aq)|| Cu2+(aq)| Cu+(aq)| Pt(s), Determine

For the Electrochemical Cell, Fe(s)| Fe²⁺(aq)|| Cu²⁺(aq)| Cu⁺(aq)| Pt(s), Determine