Consider the data given below for hypothetical reaction $A \to X$

$Time  (sec)$                     Rate $(mol\,  L^{-1} sec.^{-1})$

$0$                                      $1.60 \times 10^{-2}$

$10$                                    $1.60 \times 10^{-2}$

$20$                                    $1.60 \times 10^{-2}$

$30$                                    $1.60 \times 10^{-2}$

From the above data, the order of reaction is

The mechanism of the reaction $A + 2B \to D$ is

$2B\xrightarrow{k}{B_2}$        [Slow]

${B_2} + A \to D$          [Fast]

The rate law expression, order with respect to $A$, order with respect to $'B'$ and overall order are respectively

The rate of the simple reaction, $2NO + O_2 \to  2NO_2$, when the volume of the reaction vessel is doubled

Reaction $2A + B \to$  product,  rate law is $\frac{{ - d[A]}}{{dt}}\, = \,K[A].$ At a time when $t\, = \,\frac{{{t_{1/2}}}}{{\ln\,2}},$ concentration of the reactant is

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 ...........

The incorrect order indicated against the rate of reaction is Rate Order

$A+B\xrightarrow{K}C$

Rate                        Order