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Consider the half-cell reduction reaction : Mn2+ + 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

1. -2.69 V and no
2. -4.18 V and yes
3. +0.33 V and yes
4. +2.69 V and no

Correct answer: +0.33 V and yes

Solution

The overall cell potential is calculated by combining the given half-cell reactions. Using the formula E°cell = E°reduction (Mn2+ to Mn) - E°oxidation (Mn2+ to Mn3+), we get E°cell = -1.18 - (-1.51) = +0.33 V. A positive E° indicates the reaction is spontaneous.

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