The order of the reaction occurring by following mechanism should be

$(i)$ ${A_2} \to A + A$ (fast)

$(ii)$ $A + {B_2} \to AB + B$ (slow)

$(iii)$ $A + B \to $ (fast)

If initial concentration is reduced to its $1/4^{th}$  in a zero order reaction, the time taken for half of the reaction to complete

For the reaction $2NO_2 + F_2 \to  2NO_2F$, following mechanism has been provided :
$N{O_2} + {F_2}\xrightarrow{{slow}}N{O_2}F + F$
$N{O_2} + {F_2}\xrightarrow{{fast}}N{O_2}F$
Thus rate expression of the above reaction can be written as

Reaction rate between two substance $A$ and $B$ is expressed as following $:$ rate $= k[A ]^n[B]^m$ If the concentration of $A$ is doubled and concentration of $B$ is made half of initial concentration, the ratio of the new rate to the earlier rate will be

For reaction :

$2NO_2(g) + O_3(g) \to N_2O_5(g) + O_2(g)$

rate law is $R = K\, [NO_2]' [O_3]'$.

Which of these possible reaction mechanisms is consistent with the rate law?

Mechanism $I :$

$NO_2(g) + O_3(g) \to NO_3(g) + O_2(g)$ (slow)

$NO_3(g) + NO_2(g) \to N_2O_5(g)$ (fast)

Mechanism $II :$

$O_3(g)  \rightleftharpoons  O_2(g) + [O]$ (fast)

$NO_2(g) + [O] \to NO_3$ (slow)

$NO_3(g) + NO_2(g) \to  N_2O_5$ (fast)

Rate constant of reaction is $1.388 \times 10^{-3}\, mole^{-2}\,lit^{-2}\,sec^{-1}$ order of reaction will be