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Given below are a set of half-cell react...

Given below are a set of half-cell reactions (acidic medium) along with their `E_(@)` with respect to normal hydrogen electrode values. Using the data obtain the correct explanation to question given below. `{:(I_(2)+2e^(-)rarr2I^(-),E^(@)=0.54),(Cl_(2)+2e^(-)rarr2Cl^(-),E^(@)=1.36),(Mn^(2+)+e^(-)rarrMn^(2+),E^(@)=1.50),(Fe^(3+)+e^(-)rarrFe^(2+),E^(@)=0.77),(O_(2)+4H^(+)+4e^(-)rarr2H_(2)O,E^(@)=1.23):}`
While `Fe^(2+)` is stable, `Mn^(3+)` is not stable in acid solution because:

A

`O_(2)` oxidises `Mn^(+2)to Mn^(+3)`

B

`O_(2)` oxidises both `Mn^(+2) to Mn^(+3)` and `Fe^(+3) to Fe^(+3)`

C

`Fe^(+3)` oxidises `H_(2)O to O_(2)`

D

`Mn^(+3)` oxidises `H_(2)O to O_(2)`

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