Consider the redox reaction : \[2S{{O}_{2}}O_{3}^{2-}+{{I}_{2}}\to {{S}_{4}}O_{6}^{2-}+2{{I}^{-}}\]

\[2S{{O}_{2}}O_{3}^{2-}\] gets oxidised to \[S{{O}_{4}}O_{6}^{2-}\]

\[S{{O}_{2}}O_{3}^{2-}\] gets reduced to \[{{S}_{4}}O_{6}^{2-}\]

\[{{I}_{2}}\] gets reduced to \[{{I}^{-}}\]

\[{{I}_{2}}\] gets oxidised to \[{{I}^{-}}\]

Consider the redox reaction : \[2S{{O}_{2}}O_{3}^{2-}+{{I}_{2}}\to {{S

1.	Consider the redox reaction : \[2S{{O}_{2}}O_{3}^{2-}+{{I}_{2}}\to {{S}_{4}}O_{6}^{2-}+2{{I}^{-}}\]
A.	\[2S{{O}_{2}}O_{3}^{2-}\] gets oxidised to \[S{{O}_{4}}O_{6}^{2-}\]
B.	\[S{{O}_{2}}O_{3}^{2-}\] gets reduced to \[{{S}_{4}}O_{6}^{2-}\]
C.	\[{{I}_{2}}\] gets reduced to \[{{I}^{-}}\]
D.	\[{{I}_{2}}\] gets oxidised to \[{{I}^{-}}\]
Answer» E.

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Consider the redox reaction : \[2S{{O}_{2}}O_{3}^{2-}+{{I}_{2}}\to {{S}_{4}}O_{6}^{2-}+2{{I}^{-}}\]

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