Find the standard electrode potential of `MnO_(4)^(c-)|MnO_(2).` The standard electrode potential of `MnO_(4)^(c-)|Mn^(2+)=1.51V` and `MnO_(2)|MnO_(2)|Mn^(2+)=1.23V`.

Options

A. `-0.33V,` the reaction will not occur
B. `-0.33V,` the reaction will occur
C. `-2.69V,` the reaction will not occur
D. `-2.69V,` the reaction will occur

Answer

c

Explanation

`Mn^(2+)+e^(c-) rarr Mn," "E^(c-)=-1.18V`
`2Mn^(3+)rarr 2Mn^(3+)+2e^(c-), " "E^(c-)=-1.51V`
`ulbar(3Mn^(2+)rarr Mn+2Mn^(3+))`
`E_(cell)^(c-)=E_(red)^(c-)+E_(o x i d)^(c-)`
`=-1.18+(-1.51)=-2.69V`
Negative `EMF` reflects non`-`spontaneous cell reaction.