?The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: \(\mathrm{OCl}^{-}+\mathrm{I}^{-} \long

Chapter 14, Problem 14.33

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The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: \(\mathrm{OCl}^{-}+\mathrm{I}^{-} \longrightarrow \mathrm{OI}^{-}+\mathrm{Cl}^{-}\). This rapid reaction gives the following rate data:

(a) Write the rate law for this reaction.

(b) Calculate the rate constant with proper units.

(c) Calculate the rate when \(\left[\mathrm{OCl}^{-}\right]=2.0 \times 10^{-3} \mathrm{M}\) and \(\left[\mathrm{I}^{-}\right]=5.0 \times 10^{-4} \mathrm{M}\).

Text Transcription:

OCl - + I - \longrightarrow  OI - + Cl -

[OCl -] = 2.0 X 10-3 M

[I - ] = 5.0 X 10 - 4 M