Given below are the half-cell reactions: $Mn^{2+} + 2e^- \rightarrow Mn$ $(E^0 = -1.18 \text{ V})$; $Mn^{3+} + e^- \rightarrow Mn^{2+}$ $(E^0 = +1.51 \text{ V})$. The $E^0_{cell}$ for $3Mn^{2+} \rightarrow Mn + 2Mn^{3+}$ will be . . . . . .

• A
  $-2.69 \text{ V}$, the reaction will not occur (Non-Spontaneous)
• B
  $-2.69 \text{ V}$, the reaction will occur (Spontaneous)
• C
  $-0.33 \text{ V}$, the reaction will not occur (Non-Spontaneous)
• D
  $-0.33 \text{ V}$, the reaction will occur (Spontaneous)