Question

1. Consider the half-cell reduction reactions :
Mn2+ + 2€ → Mn, Eº=-118 V
Mn2+ → Mn3+ + é, E°=-1.51 V
The Eº for the reaction 3Mn→Mn +2Mn3, and
possibility of the forward reaction are respectively
(a) -4.18 V and yes (b) +0.33 V and yes
(c) +2.69 V and no (d) - 2.69 V and no
(NEET Kamataka)​

Answer 1

Answer:

Standard electrode potential of reaction will not change due to multiply the half-cell reactions with some numbers,

To get the main eq we have to reverse 2nd equation and add them

$e ^{3} = e ^{2} + e ^{1}$

$e ^{3} = - 18.8 + ( - 1.51)$

$e ^{3} = 2.69v$

The reaction is not possible as the ΔG will come +ve for this case and that indicates reaction is non-spontaneous.

Explanation:

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