Chemistry - Chemical Kinetics Question with Solution | TestHub

Chlorine dioxide oxidizes iodide ion in an aqueous solution to iodine and get reduced to chlorite ion.

$2Cl{O}_2(aq)+2I^{-}(aq)⟶2Cl{O}_2^{-}(aq)+I_2(aq)$

The order of the reaction with respect to $Cl{O}_2$ was determined by starting with a large excess of $I^{-}$, so that its concentration was essentially constant. Then, :

$rate=k[Cl{O}_2{]}^m[I^{-}{]}^n=k^{\prime }[Cl{O}_2{]}^m$

where $k^{\prime }=k[I^{-}{]}^n$. Given below the time and the concentration of $Cl{O}_2$taken:

Time (s) $[Cl{O}_2]$ (M)

0.00 $4.77\times 10^{-4}$

1.00 $4.31\times 10^{-4}$

2.00 $3.85\times 10^{-4}$