A voltaic cell is made by connecting two half-cells represented by the half-equations below.

\[\begin{array}{*{20}{l}} {{\text{M}}{{\text{n}}^{2 + }}{\text{(aq)}} + {\text{2}}{{\text{e}}^ - } \to {\text{Mn(s)}}}&{{E^\Theta } =  - 1.19{\text{ V}}} \\ {{\text{P}}{{\text{b}}^{2 + }}{\text{(aq)}} + {\text{2}}{{\text{e}}^ - } \to {\text{Pb(s)}}}&{{E^\Theta } =  - 0.13{\text{ V}}} \end{array}\]

Which statement is correct about this voltaic cell?

A.     Mn is oxidized and the voltage of the cell is 1.06 V.

B.     Pb is oxidized and the voltage of the cell is 1.06 V.

C.     Mn is oxidized and the voltage of the cell is 1.32 V.

D.     Pb is oxidized and the voltage of the cell is 1.32 V.

A