For a certain reaction, the rate $=k[A]^2[B]$, when the initial concentration of $A$ is tripled keeping concentration of $B$ constant, the initial rate would

Calculate the order of the reaction in $A$ and $B$

Fill up the blank :

$1.$ The rate of reaction depends on ........... step.

$2.$ In bimolecular reaction the reaction take place with ........... species and ........... .

$3.$ The order of reaction is determine by ...........

$n$ presence of $HCl$, sucrose gets hydrolysed into glucose and fructose. The concentration of sucrose was found to reduce form $0.4\,M $ to $0.2 \,M$  in $1$  hour and $0.1 \,M $ in $2$ hours. The order of the reaction is

For a reaction, $I^-+OCl^-  \to IO^-+Cl^-$ in a aqueous medium, the rate of reaction is given by $\frac{{d[{IO^ - }]}}{{dt}} = k[{I^ - }][OC{l^ - }]$ The overall order of reaction is

The hypothetical reaction : $2A + B \to C + D$ is catalyzed by $E$ as indicated in the possible mechanism below -

Step$-1$ : ${\text{A  +  E }} \rightleftharpoons AE$ (fast)

Step$-2$ :${\text{AE  +  A }} \to {A_2} + E$ (slow)

Step$-3$ :${{\text{A}}_2}{\text{ +  B }} \to {\text{D}}$ (fast)

what rate law best agrees with this mechanism