To calculate the standard electrode potential for the oxidation of Fe2+ ions to Fe3+ ions, we need to find the half-reactions and their respective standard electrode potentials. The half-reactions are as follows:1. Oxidation half-reaction: Fe2+ Fe3+ + e- Fe2+ loses an electron 2. Reduction half-reaction: Fe3+ + e- Fe2+ Fe3+ gains an electron Now, we need to find the standard electrode potentials E for these half-reactions. The standard electrode potentials are:1. E Fe2+/Fe3+ = +0.77 V for the reduction half-reaction 2. E Fe3+/Fe2+ = -0.77 V for the oxidation half-reaction The balanced chemical equation for the overall reaction is:Fe2+ Fe3+ + e-To determine if the reaction is spontaneous or non-spontaneous at standard conditions, we need to calculate the standard cell potential Ecell using the Nernst equation:Ecell = E cathode - E anode In this case, the cathode is the reduction half-reaction, and the anode is the oxidation half-reaction. Therefore, the standard cell potential is:Ecell = +0.77 V - -0.77 V = +1.54 VSince the standard cell potential Ecell is positive +1.54 V , the reaction is spontaneous at standard conditions.