The equivalent mass of iodine in the followin | vedclass

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(B) The reaction is $I_2 + 2S_2O_3^{2-} \longrightarrow 2I^{-} + S_4O_6^{2-}$.In this reaction,the oxidation state of $I$ changes from $0$ in $I_2$ to

Vedclass · Accepted Answer

$127$

Vedclass · Answer

(B) The reaction is $I_2 + 2S_2O_3^{2-} \longrightarrow 2I^{-} + S_4O_6^{2-}$.In this reaction,the oxidation state of $I$ changes from $0$ in $I_2$ to $-1$ in $I^-$.Total change in oxidation state for one molecule of $I_2$ is $2 	imes |0 - (-1)| = 2$.Thus,the valence factor $(v.f.)$ is $2$.The molar mass of $I_2$ is $2 	imes 127 = 254 \ g/mol$.The equivalent mass is calculated as $\frac{	ext{Molar mass}}{v.f.} = \frac{254}{2} = 127$.

The equivalent mass of iodine in the following reaction is $I_2 + 2S_2O_3^{2-} \longrightarrow 2I^{-} + S_4O_6^{2-}$

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