Standard reduction potentials of the half reactions are given below -F2g -2e- - 2F- aq- E- - -2-85 VCl2g -2e- 2Cl-aq - E- - -1-36 VBr2l-2e- 2Br-aq - E- - 1-06 VI2s -2e- 2I-aq - E- - -0-53 Vthe strongest oxidizing and reducing agents respectively are -

We know that Oxidising nature ∝ Standard reduction potential nbsp; reducing nature ∝ 1Standard reduction potential In the given values, F_2 has highest stand ...

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Standard XII

Chemistry

Acidic Character, Basic Character and Nature of Oxides

Standard redu...

Question

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 :

C l_{2} a n d I_{2}

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C l_{2} a n d B r^{-}

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B r_{2} a n d C l^{-}

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F_{2} a n d I^{-}

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Solution

The correct option is D $F_{2} a n d I^{-}$
We know that
Oxidising nature $\propto$ Standard reduction potential
$reducing nature \propto \frac{1}{Standard reduction potential}$

In the given values, $F_{2}$ has highest standard reduction potential. Therefore it is strongest oxidizing agent,
In the given values iodine has least standard reduction potential.
Therefore $I^{-}$ is strongest reductant,

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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^{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 (g)} + e^{-} \to 2 I_{(a q)}^{-}; E^{o} = + 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^{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) + e^{-} \to 2 B r^{-} (a q) : E^{0} = + 1.06 V

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

The strongest oxidizing and reducing agent among the given reactions are ____________ respectively.

Q. The standard reduction potentials at 298 K for the following half reactions are given,

Z n_{(a q)}^{2 +} + 2 e^{-} ⇌ Z n_{(s)}

E^{\circ}

- 0.762 V

C r_{(a q)}^{3 +} + 3 e^{-} ⇌ C r_{(s)}

E^{\circ}

- 0.740 V

2 H_{(a q)}^{+} + 2 e^{-} ⇌ H_{2 (g)}

E^{\circ}

0.000 V

F e_{(a q)}^{3 +} + e^{-} ⇌ F e_{(s)}^{2 +}

E^{\circ}

0.770 V

Which is the strongest reducing agent?

Q. The standard reduction potentials at 298 K for the following half reactions are given:

Which is the strongest reducing agent?

Z n^{2 +} (a q .) + 2 e ⇌ Z n (s); - 0.762

C r^{3 +} (a q) + 3 e ⇌ C r (s); - 0.740

2 H^{+} (a q) + 2 e ⇌ H_{2} (g); 0.00

F e^{3 +} (a q) + e ⇌ F e^{2 +} (a q); 0.770

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Standard reduction potentials of the half reactions are given below : F2(g)+2e−→2F−(aq); E∘=+2.85 V Cl2(g)+2e−→2Cl−(aq) ; E∘=+1.36 V Br2(l)+2e−→2Br−(aq) ; E∘=+1.06 V I2(s)+2e−→2I−(aq) ; E∘=+0.53 V the strongest oxidizing and reducing agents respectively are :