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The value of n in : MnO(4)^(-)+8H^(+)+n ...

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

Answer

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Find out the value of n in: MnO_(4)^(-) + 8H^(+) + "ne" rarr Mn^(2+) + 4H_(2)O

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

Knowledge Check

  • The value of n in NO_3^(-) + 4H^(+) + n e^(-) rarr 2 H_2O + NO is .

    A
    `2`
    B
    `4`
    C
    `5`
    D
    `3`

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

    A
    5
    B
    8
    C
    6
    D
    3

  • For the following reaction in the acidic solution MnO_(4)^(-)+8H^(+)+5e^(-)rarrMn^(2+)+4H_(2)O which of the following gives the true oxidation numbers of the manganese on each side of the equation ?

    A
    `+ 7` to `+6`
    B
    `+7` to `+2`
    C
    `+4` to `+2`
    D
    `-1` to `+2`

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    The value of x in the partial redox equation MnO_(4)^(-)+8H^(+)+xe^(-) hArr Mn^(2+)+4H_(2)O is

    The value of x in the partial redox equation MnO_(4)^(-)+8H^(+)+xe hArr Mn^(2+)+4H_(2)O is

    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 :

    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 the redox reaction MnO_(4)^(-) +8H^(+)+Br^(-)rarrMn^(2+)+4H_(2)O+5//2br_(2) which one is the reducing agent ?

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