Select the rate law for reaction $A + B \longrightarrow C$

Exp	$[A]$	$[B]$	Rate
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.070$	$0.80$
$3$	$0.024$	$0.035$	$0.10$
$4$	$0.012$	$0.070$	$0.80$

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

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

${B_2} + A \to D\,\left[ {Fast} \right]$

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

Differential form of the rate equation is

$\frac{{dx}}{{dt}} = k\left[ P \right]{\left[ Q \right]^{0.5}}{\left[ R \right]^{0.5}}$ 

Which statement about the above equation is wrong?

State a condition under which a bimolecular reaction is kinetically first order reaction.

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)

For the reaction, $2N_2O_5 \to 4NO_2 + O_2$ rate and rate constant are $1.02 \times 10^{-4}\, mol\,L^{-1}\,s^{-1}$ and $3.4 \times10^{-5}\,s^{-1}$ respectively. The concentration of $N_2O_5$ in $mol\,L^{-1}$ will be