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  • I have a doubt, kindly clarify. - Redox Reaction and Electrochemistry - JEE Main

The E^{0}{_{M^{3+}/M^{2+}}} values foCr,Mn,Fe\: and\: Co \: are\: -0.41,+1.57,0.77\: and\: +1.97 V respectively. For which one of these metals the change in oxidation state from +2\: to +3 i s easiest?

  • Option 1)

    Cr

  • Option 2)

    Mn

  • Option 3)

    Fe

  • Option 4)

    Co

 

Answers (1)

best_answer

As we learnt in

Oxidising Agent -

A substance that act as acceptor of electron is called oxidising agent. Cl2 itself get reduced in the process

- wherein

e.g. 2Na(s) + Cl_{2}(g)\rightarrow 2Na^{+}Cl^{-}

Cl2  act as oxidising agent

 

  and

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.

-

 

   

Cr^{2+}\mid Cr^{3+}= +0.41V

Mn^{2+}\mid Mn^{3+}= -1.57V

Fe^{2+}\mid Fe^{3+}= -0.77V

Co^{2+}\mid Co^{3+}= -1.97V

More is the value of oxidation potential more is the tendency to get oxidised. As Cr will have maximum oxidation potential value, therefore its oxidation will be easiest.


Option 1)

Cr

This option is correct.

Option 2)

Mn

This option is incorrect.

Option 3)

Fe

This option is incorrect.

Option 4)

Co

This option is incorrect.

Posted by

Aadil

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