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

Why molecularity is applicable only for elementary reactions and order is applicable for elementary as well as complex reactions ?

A student has studied the decomposition of a gas $AB _3$ at $25^{\circ} C$. He obtained the following data.

The order of the reaction is

The conversion of molecules $X$ to $Y$ follows second order kinetics. If concentration of $X$ is increased to three times how will it affect the rate of formation of $Y ?$

For the following parallel chain reaction. What will be that value of overall half-life of $A$ in minutes ?

Given that  $\left[ {\frac{{{{\left[ B \right]}_t}}}{{{{[C]}_t}}} = \frac{{16}}{9}} \right]$

$A\,\xrightarrow{{{K_1}\, = \,2\, \times \,{{10}^{^{ - 3}\,}}{S^{ - 1}}}}4B$

$A\to C$

For conversion of compound $A \rightarrow B$, the rate constant of the reaction was found to be $4.6 \times 10^{-5}\,L\, mol ^{-1}\, s ^{-1}$. The order of the reaction is $..........$