The reaction [mathrm{I}^{-}(a q)+mathrm{OCl}^{-}(a q) longrightarrow mathrm{IO}^{-}(a q)+mathrm{Cl}^{-}(a q)] is believed to occur by the following mechanism:
Question:
The reaction
\[\mathrm{I}^{-}(a q)+\mathrm{OCl}^{-}(a q) \longrightarrow \mathrm{IO}^{-}(a q)+\mathrm{Cl}^{-}(a q)\]
is believed to occur by the following mechanism:
Write the rate law for this reaction. Since the reaction is in aqueous solution, the effective concentration of water remains constant. Thus the rate of the forward reaction in the first step can be written as
\[\text { Rate }=k\left[\mathrm{H}_{2} \mathrm{O}ight]\left[\mathrm{OCl}^{-}ight]=k_{1}\left[\mathrm{OCl}^{-}ight]\]
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Step by Step Answer:
To write the rate law for the reaction we need to consider the slowest step in the mechanism ...View the full answer
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