The value of n in, `MnO_4^(-)+8H^(+)+"ne"^(-)rarrMn^(2-)+4H_2O` is

The value of n in : MnO_(4)^(-)+8H^(+)+n erarr Mn^(2+)+4H_(2)O is

In the reaction : MnO_(4)^(-)+xH^(+)+n e^(-)rarrMn^(2+)+yH_(2)O What is the value of n :

In acidic medium " MnO"_(4)^(-) is an oxidising agent as " MnO"_(4)^(-) +8H^(+)+5e^(-) rarr Mn^(2+)+4H_(2) O . If H^(+) concentration is doubled, electrode potential of the half-cell " MnO"_(4)^(-)// " Mn"^(2+), Pt will :

The E_("cell") of the reaction MnO_(4)^(-)+Fe^(+2)+H^(+)rarrMn^(2+)+H_(2)O is 0.59 V at 25^(@)C The equilibrium constant for the reaction is

For the reactions {:(MnO_(4)^(-)+8H^(+)+5e^(-)rarr Mn^(2+)4H_(2)O","E^(o) = + 1.51 V),(MnO_(2)+4H^(+)+ 2e^(-) rarr Mn^(2+)+2H_(2)O"," E^(o)= + 1.23 V ):} then for the reaction : MnO_(4)^(-) + 4H^(+) + 3e^(-) rarr MnO_(2)+2H_(2)O","E^(o)

In acid medium, MnO_(4)^(c-) is an oxidizing agent. MnO_(4)^(c-)+8H^(o+)+5e^(-) rarr Mn^(2+)+4H_(2)O If H^(o+) ion concentration is doubled, electrode potential of the half cell MnO_(4)^(c-), Mn^(2+)|Pt will

In acid medium, MnO_(4)^(c-) is an oxidizing agent. MnO_(4)^(c-)+8H^(o+)+5e^(-) rarr Mn^(2+)+4H_(2)O If H^(o+) ion concentration is doubled, electrode potential of the half cell MnO_(4)^(c-), Mn^(2+)|Pt will

Calculate the potential of an indicator electrode versus the standard hydrogen electrode, which originally contained 0.1M MnO_(4)^(-) and 0.8M H^(+) and which was treated with Fe^(2+) necessary to reduce 90% of the MnO_(4) to Mn^(2+) MnO_(4)^(-) +8H^(+) +5e rarr Mn^(2+) +H_(2)O, E^(@) = 1.51V

Calculate the potential of an indicator electrode versus the standard hydrogen electrode, which originally contained 0.1M MnO_(4)^(-) and 0.8M H^(+) and which was treated with Fe^(2+) necessary to reduce 90% of the MnO_(4) to Mn^(2+) MnO_(4)^(-) +8H^(+) +5e rarr Mn^(2+) +H_(2)O, E^(@) = 1.51V

E_(cell)^(@) for the reaction MnO_(4)^(-)+5Fe^(+2)+8H^(+)rarrMn^(+2)+5Fe^(+3)+4H_(2)O is 0.59 V at 298 K. Find the equilibrium constant