The instantaneous rate of disappearance of $MnO_4^-$ ion in the following reaction is $4.56\times10^{-3}\,Ms^{-1}$,  $2MnO_4^-+ 10I^-+ 16 H^+ \to  2 Mn^{2+} + 5I_2 + 8H_2O$ The rate of appearance $I_2$ is

If the rate of the reaction is equal to the rate constant, the order of the reaction is

The rate constant of esterification $(k) = k'\, [H_2O]$ rate constant of esterification $2.0\times 10^{-3}\,min^{-1}$ calculate  $k'$.

units of rate constant of first and zero order reactions in terms of molarity $M$ unit are respectively

Calculate the overall order of a reaction which has the rate expression

$(a)$ Rate $=k[ A ]^{1 / 2}[ B ]^{3 / 2}$

$(b)$ Rate $=k[ A ]^{3 / 2}[ B ]^{-1}$

Reaction : $2Br^{-} + H_2O_2 + 2H^{+} \to  Br_2 + 2H_2O$

take place in two steps :

$(a)$ $Br^{-} + H^{+} + H_2O_2 \xrightarrow{{slow}} HOBr + H_2O$

$(b)$ $HOBr + Br^{-} + H^{+} \xrightarrow{{fast}} H_2O + Br_2$

The order of the reaction is