If E $\circ$ for the disproportionation of Cu⁺(aq) to Cu²⁺(aq)And Cu(s)Is +0.18 V at 25^$\omicron$C,Calculate the equilibrium constant for the reaction.

Question

Quizplus · Accepted Answer

The Nernst equation is:E = E° - (RT/nF)lnQwhere E is the cell potential, E° is the standard cell potential, R is the gas constant, T is the temperature in Kelvin, n is the number of moles of electrons transferred, F is the Faraday constant, and Q is the reaction quotient.At equilibrium, E = 0, so:0 = E° - (RT/nF)lnKwhere K is the equilibrium constant.Solving for K, we get:K = exp(nFE°/RT)Substituting the given values, we get:K = exp(1 * 96485 C/mol * 0.18 V / (8.314 J/mol*K * 298 K))= 1.2 * 10^6

If E ∘\circ∘ for the Disproportionation of Cu+(aq) to Cu2+(aq)And Cu(s)Is

If E^$\circ$
for the Disproportionation of Cu⁺(aq) to Cu²⁺(aq)And Cu(s)Is