`E_(RP)^(@)` and their respective half reactions for some change are given below:
i) `Mn^(7+)(aq)+8H^(+)+5erarrMn^(2+)(aq)+4H_(2)O(l),`
`E^(@)=+1.52V`
ii) `Mn^(7+)(aq)+4H^(+)+3erarrMnO_(2)(s)+2H_(2)O(l),`
`E^(@)=+2.26V`
iii) `Mn^(7+)(aq)+2erarrMn^(5+)(aq),`
`E^(@)=+0.56V("acid med.")`
`Mn^(3+)+erarrMn^(2+)`,
`E^(@)=+1.51V("acil med.")`
v) `Mn^(4+)+erarrMn^(3+),`
`E^(@)=+0.95V("acid med.")`
Which is the least stable oxidation state of Mn?

E_(RP)^(@) and their respective half reactions for some change are given below: i) Mn^(7+)(aq)+8H^(+)+5erarrMn^(2+)(aq)+4H_(2)O(l), E^(@)=+1.52V ii) Mn^(7+)(aq)+4H^(+)+3erarrMnO_(2)(s)+2H_(2)O(l), E^(@)=+2.26V iii) Mn^(7+)(aq)+2erarrMn^(5+)(aq), E^(@)=+0.56V("acid med.") Mn^(3+)+erarrMn^(2+) , E^(@)=+1.51V("acil med.") v) Mn^(4+)+erarrMn^(3+), E^(@)=+0.95V("acid med.") The most stable oxidation state of Mn is:

E_(RP)^(@) and their respective half reactions for some change are given below: i) Mn^(7+)(aq)+8H^(+)+5erarrMn^(2+)(aq)+4H_(2)O(l), E^(@)=+1.52V ii) Mn^(7+)(aq)+4H^(+)+3erarrMnO_(2)(s)+2H_(2)O(l), E^(@)=+2.26V iii) Mn^(7+)(aq)+2erarrMn^(5+)(aq), E^(@)=+0.56V("acid med.") Mn^(3+)+erarrMn^(2+) , E^(@)=+1.51V("acil med.") v) Mn^(4+)+erarrMn^(3+), E^(@)=+0.95V("acid med.") The E^(@) for, Mn^(4+)+2erarrMn^(2+), is equal to:

Two half-reactions of an electrochemical cell are given below : MnO_(4)^(-)(aq)+8H^(+)(aq)+5e^(-) toMn^(2+)(aq)+4H_(2)O(l), E^(@)=+1.51" V" Sn^(2+)(aq) to Sn^(4+)(aq)+2e^(-),E^(@)=-0.15" V"

MnO_(4)^(-) + 8H^(+) + 5e^(-) rightarrow Mn^(2+) + 4H_(2)O , E^(@) = 1.51V MnO_(2) + 4H^(+) + 2e^(-) righarrow Mn^(2+) + 2H_(2)O E^(@) = 1.23V E_(MnO_(4)^(-)|MnO_(2)

MnO_(4)^(-) + 8H^(+) + 5e^(-) rightarrow Mn^(2+) + 4H_(2)O , E^(@) = 1.51V MnO_(2) + 4H^(+) + 2e^(-) righarrow Mn^(2+) + 2H_(2)O E^(@) = 1.23V E_(MnO_(4)^(-)|MnO_(2)

Write the appropriate Nernst equation for the following half-cell reaction: MnO_4^-(aq) +8H^+(aq)+5erarrMn^(2+)(aq)+4H_2O (I)

Write the appropriate Nernst equation for the following half-cell reaction: MnO_(4)^(-)(aq) +8H^(+) (aq) +5e to Mn^(2+)(aq) +4H_(2)O(l)

Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration. Some half cell reaction and their standard potentials are given below: MnO_(4)^(-)(aq) +8H^(+)(aq) +5e^(-) rarr Mn^(2+)(aq) +4H_(2)O(l) E^(@) = 1.51V Cr_(2)O_(7)^(2-)(aq) +14H^(+) (aq) +6e^(-) rarr 2Cr^(3+)(aq) +7H_(2)O(l), E^(@) = 1.38V Fe^(3+) (aq) +e^(-) rarr Fe^(2+) (aq), E^(@) = 0.77V CI_(2)(g) +2e^(-) rarr 2CI^(-)(aq), E^(@) = 1.40V Identify the only incorrect statement regarding quantitative estimation of aqueous Fe(NO_(3))_(2)

Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration. Some half cell reaction and their standard potentials are given below: MnO_(4)^(-)(aq) +8H^(+)(aq) +5e^(-) rarr Mn^(2+)(aq) +4H_(2)O(l) E^(@) = 1.51V Cr_(2)O_(7)^(2-)(aq) +14H^(+) (aq) +6e^(-) rarr 2Cr^(3+)(aq) +7H_(2)O(l), E^(@) = 1.38V Fe^(3+) (aq) +e^(-) rarr Fe^(2+) (aq), E^(@) = 0.77V CI_(2)(g) +2e^(-) rarr 2CI^(-)(aq), E^(@) = 1.40V Identify the only correct statement regarding quantitative estimation of aqueous Fe(NO_(3))_(2)