🤓 Based on our data, we think this question is relevant for Professor Montano's class at UIC.
We are asked to find the equilibrium constant K for the spontaneous reaction between Ni2+(aq) and Cd(s).
We will use the Gibbs Free Energy Equation to calculate the equilibrium constant. The Gibbs Free relates the potential of compounds and cell equilibrium:
In a Galvanic Cell, the Gibbs free energy is related to the potential by:
If the Eocell > 0, then the process is spontaneous (galvanic cell)
If the Eocell < 0, then the process is nonspontaneous (electrolytic cell)
ΔGo can also be expressed by the equilibrium constant Keq of the reaction.
Combining the two equations since both are equal to ΔGo gives:
n = # of e- transferred
F = Faraday’s constant = 96485 J/(mol e-)
E°cell = standard cell potential, V
R = gas constant, 8.314 J/mol e- K
T = temperature in K
Keq = equilibrium constant of the reaction
In the Gibbs Equation, we have to determine the E°cell first, as well as the anode (oxidation) and the cathode (reduction) in the concentration cell and the number of electrons transferred (n).
Compute the equilibrium constant for the spontaneous reaction between Ni2+(aq) and Cd(s).