Answer:
Weaker is the bond, greater is
the reactivity of halogenated acid.
\[\xrightarrow[\text{Decreasing}\,\text{reacticaity}]{HI>HBr>HCl}\]
Since the bond dissociation
energy decreases in the order:
\[HCl(430.5kJmo{{l}^{-1}})>HBr(363.7kJmo{{l}^{-1}})>HI(296.8kJmo{{l}^{-1}})\]therefore,
the reactivity of the halogen acids decreases in the reverse order :
\[HI>HBr>HCl\]
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