Standard reduction potential of the half reaction are given below

F_{2}\left ( g \right )+2e^{-}\rightarrow 2F^{-}\left ( aq \right );E^{0}= +2.85V

Cl_{2}\left ( g \right )+2e^{-}\rightarrow 2Cl^{-}\left ( aq \right );E^{0}= +1.36V

Br_{2}\left ( 1 \right )+2e^{-}\rightarrow 2Br^{-}\left ( aq \right );E^{0}= +1.06V

I_{2}\left ( s \right )+2e^{-}\rightarrow 2I^{-}\left ( aq \right );E^{0}= +0.53V

The strongest oxidising and reducing agents respectively are:

  • Option 1)

    F_{2}\ and\ I^{-}

  • Option 2)

    Br_{2}\ and\ CI^{-}

  • Option 3)

    Cl_{2}\ and\ Br^{-}

  • Option 4)

    Cl_{2}\ and\ I_2

 

Answers (1)
D Divya Saini

 

Standard Electrode Potential -

If concentration of each species taking part in the electrode reaction is unity and further the reaction is carried out at 298 K, then the potential of each electrode is said to be the standard electrode potential.

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Standard Electrode Potential -

If concentration of each species taking part in the electrode reaction is unity and further the reaction is carried out at 298 K, then the potential of each electrode is said to be the standard electrode potential.

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 more negative the value of the reduction  potential, stronger will be reducing agen, thus Iis strongest reducing agent more positive value of reduction potential shows good oxidising properties thus strongest oxidising agent is F2.


Option 1)

F_{2}\ and\ I^{-}

Correct

Option 2)

Br_{2}\ and\ CI^{-}

Incorrect

Option 3)

Cl_{2}\ and\ Br^{-}

Incorrect

Option 4)

Cl_{2}\ and\ I_2

Incorrect

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