For the reaction 5 Br^ - (aq)+BrO_3^ - (aq)+6 H^ + (aq) arrow 3...

For the reaction $5 \mathrm{Br}^{-}(\mathrm{aq})+\mathrm{BrO}_3^{-}(\mathrm{aq})+6 \mathrm{H}^{+}(\mathrm{aq}) \rightarrow 3 \mathrm{Br}_2(\mathrm{aq})+3 \mathrm{H}_2 \mathrm{O}(\mathrm{l})$ the rate expression was found to be $-\mathrm{d}$\left[\mathrm{BrO}}_{3}{ }^{-}\right] / $\mathrm{dt}=\mathrm{k}$ \left[\mathrm{Br}^{-}\right] \left[\mathrm{H}^{+}\right]^2 \left[\mathrm{BrO}}_{3}{ }^{-}\right]$Which of the following statement/s is /are correct? I. Doubling the initial concentration of all the reactants will increase the reaction rate by a factor of 8 II. Unit of rate constant of the reaction in a buffer solution is$\min ^{-1}III. Doubling the concentration of all the reactants at the same time will increase the reaction rate by a factor of 16 IV. rate of conversion of \mathrm{BrO}}_{3}^{-}and rate of formation of \mathrm{Br}^{-}are the same