Question

When the reaction \[ \mathrm{I}^{-}(a q)+\mathrm{OCl}^{-}(a q) \rightarrow \mathrm{IO}^{-}(a q)+\mathrm{Cl}^{-}(a q) \] was studied, the following data were obtained: \begin{tabular}{|c|c|c|} \hline\( \left[\mathrm{I}^{-}\right](\mathrm{mol} / \mathrm{L}) \) & {\( \left[\mathrm{OCl}^{-}\right]_{0}(\mathrm{~mol} / \mathrm{L}) \)} & Initial Rate \( (\mathrm{mol} / \mathrm{L} \cdot \mathrm{s}) \) \\ \hline 0.12 & 0.14 & 0.080 \\ \hline 0.060 & 0.14 & 0.040 \\ \hline 0.030 & 0.070 & 0.010 \\ \hline 0.24 & 0.070 & 0.080 \\ \hline \end{tabular} What is the rate law? Rate \( = \) \( \square \)

          When the reaction
\[
\mathrm{I}^{-}(a q)+\mathrm{OCl}^{-}(a q) \rightarrow \mathrm{IO}^{-}(a q)+\mathrm{Cl}^{-}(a q)
\]
was studied, the following data were obtained:
\begin{tabular}{|c|c|c|}
\hline\( \left[\mathrm{I}^{-}\right](\mathrm{mol} / \mathrm{L}) \) & {\( \left[\mathrm{OCl}^{-}\right]_{0}(\mathrm{~mol} / \mathrm{L}) \)} & Initial Rate \( (\mathrm{mol} / \mathrm{L} \cdot \mathrm{s}) \) \\
\hline 0.12 & 0.14 & 0.080 \\
\hline 0.060 & 0.14 & 0.040 \\
\hline 0.030 & 0.070 & 0.010 \\
\hline 0.24 & 0.070 & 0.080 \\
\hline
\end{tabular}

What is the rate law?
Rate \( = \) \( \square \)

When the reaction

I^-(a q)+OCl^-(a q) →IO^-(a q)+Cl^-(a q)

was studied, the following data were obtained:

[I^-](mol / L) [OCl^-]0( mol / L) Initial Rate (mol / L·s)

0.12 0.14 0.080

0.060 0.14 0.040

0.030 0.070 0.010

0.24 0.070 0.080

What is the rate law?
Rate = □

Added by Tammy J.

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