Consider the half-cell reduction reactionMn2++2e-→Mn,E°=-1.18 V Mn2+→Mn3++e-,E°=-1.51 V The E° for the reaction 3Mn2+→Mn0+2Mn3+ ,and possibility of the forward reaction are respectively

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Consider the half-cell reduction reaction

${Mn}^{2 +} + 2 e^{-} \to Mn, E ° = - 1.18 V {Mn}^{2 +} \to {Mn}^{3 +} + e^{-}, E ° = - 1.51 V The E ° for the reaction 3 {Mn}^{2 +} \to {Mn}^{0} + 2 {Mn}^{3 +}, and possibility of the forward reaction are respectively$

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$- 2.69 V and no$

$+ 0.33 V and yes$

$+ 2.69 V and no$

$- 4.18 V and yes$

answer is D.

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Detailed Solution

${Mn}^{2 +} + 2 e^{-} \to Mn E ° = - 1.18 V 2 {Mn}^{2 +} \to 2 {Mn}^{3 +} + 2 e^{-} E ° = - 1.51 V For the cell, 3 {Mn}^{2 +} \to Mn + 2 {Mn}^{3 +} E ° = - 2.69 V Since the E ° value is negative, so the process is non - spantaneous$