Chlorine dioxide, $Cl{O}_2,$ is a reddish$-$yellow gas that is soluble in water. In basic solution it gives $Cl{O}_3^{-}$and $Cl{O}_2^{-}$ions.

$2Cl{O}_2(aq)+2O{H}^{-}(aq)Cl{O}_3^{-}(aq)+Cl{O}_2^{-}(aq)+H_{2}O(l)$

To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of $Cl{O}_2$ was determined.

Initial Concentration Initial Concentration Initial Rate

of $Cl{O}_2(mo\frac{l}{L})$ of $O{H}^{-}(mo\frac{l}{L})($mol$/($L$.$s$))$

Exp. $1,0\mathrm{.}18$

$2\mathrm{.}6{10}^{-2},0\mathrm{.}193$

Exp. $2$

$6\mathrm{.}0{10}^{-2}$

$2\mathrm{.}6{10}^{-2}$

$2\mathrm{.}14{10}^{-2}$

Exp. $3$

$6\mathrm{.}0{10}^{-2}$

$7\mathrm{.}8{10}^{-2}$

$6\mathrm{.}43{10}^{-2}$

a Obtain the rate law.

$($Use $k$ for the rate constant.$)$

Rate law $=$

b Choose the units of the rate constant.

$\frac{L^2}{mo{l}^2*s}$

$s^{-1}$

$mo\frac{l}{L}$

$mo\frac{l}{L*s}$

C Obtain the value of the rate constant.

Rate constant $=1379\mathrm{.}6\frac{L^2}{mo{l}^2*s}$