Redox Reactions - Result Question 19
####21. Standard reduction potentials of the half reactions are given below :
$F_2(g)+2 e^{-} \to 2 F^{-}(aq) ; E^{\circ}=+2.85 V$
$Cl_2(g)+2 e^{-} \to 2 Cl^{-}(aq) ; E^{\circ}=+1.36 V$
$Br_2(l)+2 e^{-} \to 2 Br^{-}(aq) ; E^{\circ}=+1.06 V$
$I_2(s)+2 e^{-} \to 2 I^{-}(aq) ; E^{\circ}=+0.53 V$ The strongest oxidising and reducing agents respectively are :
(a) $F_2$ and $I^{-}$
(c) $Cl_2$ and $Br^{-}$
(b) $Br_2$ and $Cl$
(d) $Cl_2^{2}$ and $I_2$
[2012 M]
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Solution:
- (a) $F_2$ is the strongest oxidising agent as it has highest reduction potential while $I^{-}$is the strongest reducing agent since it has lowest reduction potential.
Higher the value of reduction potential, higher will be the oxidising power whereas the lower the value of reduction potential higher will be the reducing power.
