Consider the following standard electrode potentials and calculate the equilibrium constant at 25° C for the indicated disproportion nation reaction:\[3M{{n}^{2+}}(aq)\xrightarrow{{}}Mn(s)+2M{{n}^{3+}}(aq)\]\[M{{n}^{3+}}\left( aq \right)+{{e}^{-}}\xrightarrow{{}}M{{n}^{2+}}\left( aq \right);{{E}^{{}^\circ }}=1.51\text{ }V\]\[M{{n}^{2+}}(aq)+2{{e}^{-}}\xrightarrow{{}}Mn(s);E{}^\circ =-1.185V\]

• A. \[1.2\times {{10}^{-43}}\]
• B. \[2.4\times {{10}^{-73}}\]
• C. \[6.3\times {{10}^{-92}}\]
• D. \[1.5\times {{10}^{-62}}\]