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Given below are the half - cell reactions : $\;Mn^{2+}+2e^{-} \to Mn\;:E^{0}=-1.18\;V\;$ $\qquad \qquad \qquad \qquad\;$ $\qquad \qquad \qquad \qquad\;$ $\;2(Mn^{3+}+e^{-} \to Mn^{2+})\;:E^{0}=+1.51\;V\;$ $\qquad \qquad \qquad \qquad\;$ $\qquad \qquad \qquad \qquad\;$ $\qquad \qquad \qquad \qquad \qquad \qquad \qquad \qquad \qquad\;$ The $\;E^{0}\;$ for $\;3Mn^{2+} \to Mn +2Mn^{+}\;$

(a) -2.69 V ; The reaction will not occur \[\](b) -2.69 V ; The reaction will occur\[\](c) -0.33 V ; The reaction will not occur\[\](d) -2.69 V ; The reaction will occur
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