Which of the following is correct ?

The rate law expression for the reaction $aA + bB \to P$ is rate $= K [A]^p [B]^q$ The order of the reaction is

For the reaction,

$2{N_2}{O_5}\, \to \,4N{O_2}\, + \,{O_2}$

the rate of reaction is

Assuming the reaction

$2NO(g) + Cl_2(g) \longrightarrow 2NOCl(g)$

occurs in a single elementary step, we can say that

The experimental data for decomposition of $N _{2} O _{5}$

$\left[2 N _{2} O _{5} \rightarrow 4 NO _{2}+ O _{2}\right]$

in gas phase at $318 \,K$ are given below:

$(i)$ Plot $\left[ N _{2} O _{5}\right]$ against $t$

$(ii)$ Find the half-life period for the reaction.

$(iii)$ Draw a graph between $\log \left[ N _{2} O _{5}\right]$ and $t$

$(iv)$ What is the rate law $?$

$(v)$ Calculate the rate constant.

$(vi)$ Calculate the half-life period from $k$ and compare it with $(ii)$.

The reaction $2 A + B _{2} \rightarrow 2 AB$ is an elementary reaction.

For a certain quantity of reactants, if the volume of the reaction vessel is reduced by a factor of $3,$ the rate of the reaction increases by a factor of $.....$. (Round off to the Nearest Integer).