Chapter 11, Problem 82QAP

When a base is added to an aqueous solution of chlorine dioxide gas, the following reaction occurs:

$2{\text{ClO}}_2\left(aq\right)+2{\text{OH}}^{-}\left(aq\right)\to {\text{ClO}}_3{}^{-}\left(aq\right)+{\text{ClO}}_2{}^{-}\left(aq\right)+{\text{H}}_2\text{O}$ The reaction is first-order in ${\text{OH}}^{-}$ and second-order for ${\text{ClO}}_{\text{2}}$ Initially, when $\left[{\text{ClO}}_{\text{2}}\right]=0.010M$ and $\left[{\text{OH}}^{-}\right]=0.030M$, the rate of the reaction is $6.00\times {10}^{-4}\text{mol}/\text{L}\cdot \text{s}$. What is the rate of the reaction when 50.0 mL of 0.200 M ${\text{ClO}}_{\text{2}}$ and 95.0 mL of 0.155 M NaOH are added?