1. The problem statement, all variables and given/known data Calculate the cell potential (ECell) of an electrochemical cell with Mg/Mg^2+, and Fe/Fe^2+ electrodes. [Mg^2+] and [Fe^2+] = 1.00 M. Fe^2+(aq) + 2e^- --> Fe(s) = -0.45V Mg^2+(aq) + 2e^- --> Mg(s) = -2.37 V a) 1.90 b) 1.92 c) 1.94 d) 2.82 e) 2.80 2. Relevant equations ECell = EReduction + EOxidation 3. The attempt at a solution I believe the answer is B as I believe because the Mg having a lower value of V will have it's sign changed to form a positive value (oxidation). Is this correct?