The standard reduction potential of Fe3+ to Fe2+ is +0.77 V. This value is found in standard reduction potential tables and represents the potential difference when one mole of Fe3+ ions gains one mole of electrons to form one mole of Fe2+ ions under standard conditions 1 M concentration, 25C, and 1 atm pressure .To determine the voltage output of a standard electrochemical cell with an iron anode and a copper cathode, we need to consider the half-reactions involved:1. Oxidation half-reaction at the anode Iron :Fe s Fe2+ aq + 2eThe standard reduction potential for this reaction is -0.44 V. However, since it is an oxidation reaction, we need to reverse the sign, making it +0.44 V.2. Reduction half-reaction at the cathode Copper :Cu2+ aq + 2e Cu s The standard reduction potential for this reaction is +0.34 V.Now, we can calculate the overall cell potential E_cell using the Nernst equation:E_cell = E_cathode - E_anodeE_cell = +0.34 V - +0.44 V = -0.10 VThe voltage output of the standard electrochemical cell with an iron anode and a copper cathode is -0.10 V. The negative sign indicates that the reaction is not spontaneous under standard conditions.