The standard reduction potential, E°, for the half reaction O2 (g) + 2 H+ + 2 e- → 2 H2O2 (aq) has a value of 0.68 V. Determine the value of the standard reduction potential for the half reaction below. O2 (g) + 4 H+(aq) + 2 e- → 2 H2O (l)

Not a  mixture of two common elements that can be separated by physical means.

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.