The instantaneous rate of disappearance of MnO_4^- ion in the following reaction is 4.56 × 10^-3 Ms^-1; 2 MnO_4^-+10 I^-+16 H^+ → 2 Mn^2++ 5 I_2+8…

The instantaneous rate of disappearance of $\displaystyle \mathrm{MnO}_4{ }^{-}$ion in the following reaction is $$\begin{aligned} & 4.56 \times 10^{-3} \mathrm{Ms}^{-1} \\ & 2 \mathrm{MnO}_4^{-}+10 \mathrm{I}^{-}+16 \mathrm{H}^{+} \rightarrow 2 \mathrm{Mn}^{2+}+ \\ & 5 \mathrm{I}_2+8 \mathrm{H}_2 \mathrm{O} \end{aligned} $$ The rate of appearance $\displaystyle \mathrm{I}_2$ is :