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Coper metal can reduce Fe^(2+) in acidic...

Coper metal can reduce `Fe^(2+)` in acidic medium.

Text Solution

Verified by Experts

The correct Answer is:
F
It is `Fe` which can reduce `Cu^(2+)` to `Cu`.
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Copper metal reduces Fe^(2+) in an acid medium.

A given amount of Fe^(2+) is oxidised by x mol of MnO_4^– in acidic medium. Calculate mol of Cr_2O_7^(2–) required same amount of Fe^(2+) in acidic medium

Knowledge Check

  • Formic acid can reduce

    A
    Tollen's reagent
    B
    Mercuric chloride
    C
    Potassium permanganate
    D
    all

  • Formic acid can reduce

    A
    Tollen's reagent
    B
    Mercuric chloride
    C
    `KMnO_(4)`
    D
    All of these

  • Assertion : In acid solution, permanganate is reduced to Mn^(2+) by an excess of reducing agent. Reason : MnO_(4)^(-) reduced in Mn^(2+) in acidic medium and the product in the presence of an excess of permanganate is MnO_(2) .

    A
    If both assetion and reason are true and the reason is the correct explanation of the assertion.
    B
    If both assertion and reason are ture but reason is not the correct explanation of the assertion.
    C
    If assertion is true but reason is false.
    D
    If assertion is false but reason is true.

    • Similar Questions

    Explore conceptually related problems

    How many coulombs of electricity is required to reduce 1 mole of Cr_2O_7^(2-) in acidic medium?

    If equal volumes of 0.1 M KMnO_(4) and 0.1 M K_(2)Cr_(2)O_(7) solutions are allowed to oxidise Fe^(2+) to Fe^(3+) in acidic medium, then Fe^(2+) oxidised will be:

    Statements 1:Moles of KmnO_(4) required for oxidation of Fe^(+2) in acidic and basic medium will be different. Statement 2: Final oxidation state to which Mn^(+7) will be reduced will be different in case of acidic and basic medium.

    The mililitres of 0.2M KMnO_(2) required for the complete oxidation of 0.1 mol Fe^(2+ ) in acidic medium is -

    In which of the following cases H_(2)O_(2) can act as a reducing agent in an acidic medium? (Dydrogen peroxide acts both as an oxidising and as well as a reducing agent depending upon the nature of the reacting species.)

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