A) \[{{I}_{2}}\] will be reduced to \[{{I}^{-}}\]
B) There will be no redox reaction
C) \[{{I}^{-}}\] will be oxidised to \[{{I}_{2}}\]
D) \[F{{e}^{2+}}\] will be oxidised to \[F{{e}^{3+}}\]
Correct Answer: C
Solution :
[c] \[2{{I}^{-}}\xrightarrow[{}]{{}}{{I}_{2}}+2{{e}^{-}}\](Oxidation half-reaction) |
\[E_{oxi.}^{o}=-0.536\,V.\] |
\[F{{e}^{3+}}+{{e}^{-}}\xrightarrow[{}]{{}}F{{e}^{2+}}\](Reduction half-reaction) |
\[{{E}^{o}}={{E}^{o}}_{oxi}+{{E}^{o}}_{red}\] |
\[=+ve\] |
So, reaction will take place. |
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