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Standard reduction potentials of the half reactions are given below:

F2(g) + 2e- \rightarrow 2F-(aq) ; Eo = +2.85 V

Cl2(g) + 2e- \rightarrow 2Cl-(aq); Eo = +1.36 V

Br2(I) + 2e- \rightarrow 2Br- (aq); Eo = +1.06 V

I2(s) + 2e- \rightarrow 2I- (aq) ; Eo = +0.53 V

The strongest oxidizing and reducing agents respectively are:

  • Option 1)

    Br2 and Cl-

  • Option 2)

    Cl2 and Br-

  • Option 3)

    Cl2 and I2

  • Option 4)

    F2 and I-

 

Answers (1)

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


Option 1)

Br2 and Cl-

this option is incorrect.

Option 2)

Cl2 and Br-

this option is incorrect.

Option 3)

Cl2 and I2

this option is incorrect.

Option 4)

F2 and I-

this option is correct.

Posted by

Sabhrant Ambastha

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