Calculate E_cell for an Electrochemical Cell Based on the Two $\to$

Calculate E_cell for an electrochemical cell based on the two half-reactions given below when the reaction occurs in an acidic aqueous solution in which the pH is buffered at 4.00 and [MnO₄^-] = 1.80 M and [Fe²⁺] = 0.0220 M.Use the smallest whole-number coefficients possible when balancing the overall reaction. MnO₄^- + 4 H⁺ + 3e^- $\to$ MnO₂ + 2 H₂O $\quad$ +1.673 V
Fe²⁺ + 2 e^- $\to$ Fe $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ -0.447 V

A) +2.10 V
B) +0.964 V
C) +1.21 V
D) +1.86 V
E) +2.38 V