3. Use the following data to determine the rate law and the rate constant for the reaction 2 ClO₂(aq) + 2 OH⁻(aq) → ClO₃⁻(aq) + ClO₂⁻(aq) + H₂O(l) | Initial [ClO₂]₀ (M) | 0.050 | 0.100 | 0.100 | |---|---|---| | Initial [OH⁻]₀ (M) | 0.200 | 0.200 | 0.100

3. Use the following data to determine the rate law and the rate constant for the reaction
\[
2 \mathrm{ClO}_{2}(\mathrm{aq})+2 \mathrm{OH}^{-}(\mathrm{aq}) \rightarrow \mathrm{ClO}_{3}^{-}(\mathrm{aq})+\mathrm{ClO}_{2}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) .
\]
\begin{tabular}{|l|c|c|c|}
\hline Initial \( \left[\mathrm{ClO}_{2}\right]_{0}(\mathrm{M}) \) & 0.050 & 0.100 & 0.100 \\
\hline Initial \( \left[\mathrm{OH}^{-}\right]_{0}(\mathrm{M}) \) & 0.200 & 0.200 & 0.100 \\
\hline Initial rate \( (\mathrm{mol} /(\mathrm{L} \cdot \mathrm{min})) \) & 6.90 & 27.6 & 13.8 \\
\hline
\end{tabular}