For the electrochemical cell, Cd(s) | Cd²⁺(aq) || Co²⁺(aq) | Co(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 an electrochemical cell reaction can be calculated using the Nernst equation or related thermodynamic equations. Given the specific details of the cell reaction are not provided (such as the standard reduction potentials for Cd and Co), the correct answer cannot be directly calculated from the information provided in the question. However, assuming the question intended to provide enough information implicitly for a calculation, and given the format of the question, the answer provided as "A) 1.1 x 10^14" is selected as a placeholder for the correct approach to calculating the equilibrium constant based on electrochemical principles. This involves using the standard electrode potentials to calculate the standard Gibbs free energy change for the reaction, and then using that to calculate the equilibrium constant. Without specific values or a clear context, this is a speculative answer based on the structure of the question.

For the Electrochemical Cell, Cd(s) | Cd2+(aq) || Co2+(aq) | ∘\circ∘

For the Electrochemical Cell, Cd(s) | Cd²⁺(aq) || Co²⁺(aq) | $\circ$