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 7.000 and [BrO₃^-] = 0.880 M,[Cl^-] = 0.144 M,and = 0.260 atm.Use the smallest whole-number coefficients possible when balancing the overall reaction. BrO₃^- + 6 H⁺ + 5 e^- $\to$ Br₂ + 3 H₂O +1.52 V
Cl₂ + 2 e^- $\to$ 2 Cl^-
+1) 36 V

A) "+0.69 V"
B) "-0.37 V"
C) "+2.35 V"
D) "+0.12 V"
E) "-0.27 V"