2Cu+ (aq) → Cu (s) + Cu+ (aq) 2Cu+ (𝑎𝑞) → Cu (𝑠) + Cu+ (𝑎𝑞) is +0.36 V at 298 K. The equilibrium constant of the reaction is

The Nernst equation can be used to find the equilibrium constant (K) of a reaction. The Nernst equation is:

E = E° - (RT/nF) * lnQ

where: 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 in the reaction, F is the Faraday constant, and Q is the reaction quotient.

In this case, we are given E° = +0.36 V, T = 298 K, and we are trying to find K (which is Q at equilibrium). The reaction involves the transfer of one electron, so n = 1.

R is the gas constant, which is 8.314 J/(mol*K) and F is the Faraday constant, which is 96485 C/mol.

Rearranging the Nernst equation to solve for lnQ gives:

lnQ = nF(E - E°) / RT

At equilibrium, E = 0, so the equation simplifies to:

lnK = -nF*E° / RT

Substituting the given values into the equation gives:

lnK = -(1)(96485)(0.36) / (8.314)(298)

Solving this gives lnK = -13.03

Taking the antilogarithm of both sides gives:

K = e^(-13.03) = 2.18 x 10^-6

So, the equilibrium constant of the reaction is approximately 2.18 x 10^-6.