Standard reduction potentials of the half reactions are given belowF2g -2e- -2F-aq- E0 -2-85 VCl2g -2e- -2Cl- aq- E0 -1-36 VBr2l -2e- -2Br- aq- E0 -1-06 VI2s -2e- -2I- aq- E0 -0-53 VThe strongest oxidising and reducing agents respectively are-AIPMT 2012 Mains

Because of high standard reduction potential of F_2, it readily reduces to F^−. nbsp;So it oxidises other elements strongly. So, it is the strongest oxidising ...

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Standard redu...

Question

Standard reduction potentials of the half reactions are given below
$F_{2} (g) + 2 e^{-} \to 2 F^{-} (a q); E^{0} = + 2.85 V$
$C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q); E^{0} = + 1.36 V$
$B r_{2} (l) + 2 e^{-} \to 2 B r^{-} (a q); E^{0} = + 1.06 V$
$I_{2} (s) + 2 e^{-} \to 2 I^{-} (a q); E^{0} = + 0.53 V$

The strongest oxidising and reducing agents respectively are:

 AIPMT 2012 Mains

F_{2}

and

I^{-}

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C l_{2}

and

B r^{-}

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B r_{2}

and

C l^{-}

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C l_{2}

and

I_{2}

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Solution

The correct option is A $F_{2}$ and $I^{-}$
Because of high standard reduction potential of $F_{2}$ , it readily reduces to $F^{-}$ . So it oxidises other elements strongly. So, it is the strongest oxidising agent.
$I_{2}$ has the lowest standard reduction potential here. $I^{-}$ oxidises itself strongly and reduces others. So, it is a strong reducing agent.
Hence, option (a) is correct.

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Similar questions

Q. Standard reduction potentials of the half reactions are given below

F_{2} (g) + 2 e^{-} \to 2 F^{-} (a q); E^{0} = + 2.85 V

C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q); E^{0} = + 1.36 V

B r_{2} (l) + 2 e^{-} \to 2 B r^{-} (a q); E^{0} = + 1.06 V

I_{2} (s) + 2 e^{-} \to 2 I^{-} (a q); E^{0} = + 0.53 V

The strongest oxidising and reducing agents respectively are:

Q. Standard reduction potentials of the half reactions are given below :

F_{2 (g)} + 2 e^{-} \to 2 F^{-} (_{a q)}; E^{\circ} = + 2.85 V

C l_{2 (g)} + 2 e^{-} \to 2 C l_{(a q)}^{-}; E^{\circ} = + 1.36 V

B r_{2 (l)} + 2 e^{-} \to 2 B r_{(a q)}^{-}; E^{\circ} = + 1.06 V

I_{2 (s)} + 2 e^{-} \to 2 I_{(a q)}^{-}; E^{\circ} = + 0.53 V

the strongest oxidizing and reducing agents respectively are :

Q. Choose the correct option(s) for the given half cell reactions:

F_{2} (g) + 2 e^{-} \to 2 F^{-} (a q); E^{0} = 2.87 V C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q); E^{0} = 1.36 V F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{0} = 0.77 V

Q. Standard reduction potentials of the half reactions are given below

F_{2 (g)} + 2 e^{-} \to 2 F_{(a q)}^{-}

;

E^{o} = + 2.85 V

C l_{2 (g)} + 2 e^{-} \to 2 C l_{(a q)}^{-}

;

E^{o} = + 1.36 V

B r_{2 (l)} + 2 e^{-} \to 2 B r_{(a q)}^{-}

;

E^{o} = + 1.06 V

I_{2 (s)} + 2 e^{-} \to 2 I_{(a q)}^{-}

;

E^{o} = + 0.53 V

The strongest oxidising and reducing agents respectively are:

Q. The values of

E^{0}

of some of the reactions are given below:

I_{2} (g) + 2 e^{-} \to 2 I^{-} (a q); E^{0} = + 0.54 V

C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q); E^{0} = + 1.36 V

F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{0} = + 0.76 V

C e^{4 +} (a q) + e^{-} \to C e^{3 +} (a q); E^{0} = + 1.60 V

S n^{4 +} (a q) + 2 e^{-} \to S n^{2 +} (a q); E^{0} = + 0.15 V

Which of the following statement is/are true?

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