If $‘a’$ is the initial concentration of the reactant, the half-life period of the reaction of $n^{t h}$ order in inversely proportional to

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

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

Consider the reaction between chlorine and nitric oxide

$Cl _{2}( g )+2 NO ( g ) \rightarrow 2 NOCl ( g )$

On doubling the concentration of both reactants, the rate of the reaction increases by a factor of $8 .$ However, if only the concentration of $C l_{2}$ is doubled, the rate increases by a factor of $2 .$ The order of this reaction with respect to $NO$ is :

The elementary reaction $2SO_2(g) + O_2(g) \to 2SO_3(g)$ is carried out in $1\, dm^3$ vessel and $2\,dm^3$ vessel separately. The ratio of the reaction velocities will be

For a reaction whose rate expression is : Rate $ = k{[A]^{1/2}}{[B]^{3/2}}$, the order would be