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]

The charge required for reducing 1 mole of MnO_4^(-) to Mn^(2+) is

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 .

The magnitude of the change in oxidising power of the MnO_4^(-)//Mn^(2+) couple is x xx 10^(-4)V , if the H^(+) concentration is decreased from 1M to 10^(-4) M at 25^(@)C . (Assume concentration of MnO_4^(-) and Mn^(2+) to be same on change in H^(+) concentration ) . The value of x is ___________. (Rounded off to the nearest integer ) [Given : (2.303 RT)/(F) = 0.059 ]

How many faradays are required to reduce 1 mol of MnO_4^(-) to Mn^(2+) ?

What is the hybridisation of Mn in K_(2)MnO_(4) ?