To calculate the equilibrium constant K for the given reaction, we first need to determine the standard cell potential Ecell for the reaction. The overall reaction can be obtained by combining the two half-reactions:1. Cu2+ aq + 2 e- -> Cu s E = +0.34 V2. Zn s -> Zn2+ aq + 2 e- E = +0.76 V reverse the second half-reaction Add the two half-reactions:Cu2+ aq + Zn s -> Zn2+ aq + Cu s Now, add the standard potentials for the two half-reactions to get the standard cell potential Ecell :Ecell = E Cu2+/Cu + E Zn/Zn2+ Ecell = +0.34 V + +0.76 V Ecell = +1.10 VNow, we can use the Nernst equation to calculate the equilibrium constant K . The Nernst equation is:Ecell = RT/nF * ln K Where:Ecell = standard cell potential +1.10 V R = gas constant 8.314 J/molK T = temperature assuming 298 K n = number of electrons transferred 2 in this case F = Faraday's constant 96485 C/mol Rearrange the equation to solve for K:ln K = nF * Ecell / RT Now, plug in the values:ln K = 2 * 96485 C/mol * 1.10 V / 8.314 J/molK * 298 K ln K 50.71Now, take the exponential of both sides to solve for K:K e^50.71 K 6.2 10^21The equilibrium constant K for the reaction Cu2+ aq + Zn s -> Zn2+ aq + Cu s is approximately 6.2 10^21.