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`.

What is the standard electrode potential for the electrode, MnO_4^-//MnO_2 in an acid solution? E_(MnO_4^-,Mn^(2+))^@=1.51 V, E_(MnO_2,Mn^(2+))^@=1.23V

If /_\G^(@) for the half cell MnO_4^(-)"|"MnO_2 in an acid solution is -xF; then find the value of x.(Given: E_(MnO_4^(-)"|"Mn^(2+))^(@)=1.5V,E_(MnO_2"|"Mn^(2+))^(@)=1.25V )

If /_\G^(@) for the half cell MnO_4^(-)"|"MnO_2 in an acid solution is -xF then find the value of x.(Given: E_(MnO_4^(-)"|"Mn^(2+))^(@)=1.5V,E_(MnO_2"|"Mn^(2+))^(@)=1.25V )

Find the oxidation number of Mn in MnO_(4)^(2-) .

Find change in electrode potential of E_((MnO_4^-)//Mn^(2+)), if [ H^+ ] change from 1M to 10^(-4) M [Given RT/F = 0.059 & [ MnO_4^- ] = [ Mn^(2+) ] = 1M]