Given the relationship between the standard cell potential (ecell) and equilibrium constant (k) for a ink, where r is ideal gas consta nt 8.314 j rt redox reaction occurring in the cells is given by: ecell mol-; t is temperature in kelvins (i. e. 25 °c 298.15 k); and f is faradays constant 96,485 c mol nf referring to the provided table of electrode potentials, calculate the equilibrium constant k for the oxidation of copper in the following reaction: cu (s) +2 h* (aq)cu(aq) +h2 (g) (5 marks)

The total number of electrons is 14

Answerthe half-reaction having the greatest tendency to occur at the anode:     i₂(aq) + 2e⁻  ⇄ 2i⁻  ;   e = +0.53 v======oxidation occurs at the anode. we must therefore find the half-reaction with the greatest tendency to oxidize.the given values of e are reduction potentials (the form of the half-reactions are of reduction).the lower the reduction potential, the higher the potential to oxidize. the half-cell with the lowest reduction potential will have the greatest tendency to oxidize at the anode.the half-reaction having the greatest tendency must be    i₂(aq) + 2e⁻  ⇄ 2i⁻    e = +0.53 vbecause its reduction potential is the lowest out of the three.