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Charge in faradays needed to reduce or oxidise a given amount of a species

This type of question, asked 5 times: 2021 Paper 25, 28 Jun 2022, 26 Jul 2022, 31 Jan 2024, 1 Feb 2024. All 5 questions below, oldest first.

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  1. Question 1

    2021 Paper 25

    52
    Consider the following reaction MnO4−+8H++5e−→Mn+2+4H2O,E∘=1.51 VMnO_{4}^{-}+ 8H^{+}+ 5e^{-}\rightarrow Mn^{+ 2}+ 4H_{2}O,E^{\circ}= 1.51\text{ }V. The quantity of electricity required in Faraday to reduce five moles of MnO4−MnO_{4}^{-}is

  2. Question 2

    28 Jun 2022

    57
    The quantity of electricity in Faraday needed to reduce 1 mol1\text{ }mol of Cr2O72−Cr_{2}O_{7}^{2 -} to Cr3+Cr^{3 +} is

  3. Question 3

    26 Jul 2022

    57
    The amount of charge in FF (Faraday) required to obtain one mole of iron from Fe3O4Fe_{3}O_{4} is (Nearest Integer)

  4. Question 4

    31 Jan 2024

    60
    One Faraday of electricity liberates x×10−1x \times10^{- 1} gram atom of copper from copper sulphate, xx is _____ .

  5. Question 5

    1 Feb 2024

    147
    The amount of electricity in Coulomb required for the oxidation of 1 mol1\text{ }mol of H2OH_{2}O to O2O_{2} is ______ ×105C\times10^{5}C.