The following data is given for reaction between $A$ and $B$

$S.NO.$	$[A]$    $mol.L^{-1}$	$[B]$    $mol.L^{-1}$	$Rate$    $mol.L^{-1}\,sec^{-1}$
$I$	$1 \times 10^{-2}$	$2 \times 10^{-2}$	$2 \times 10^{-4}$
$II$	$2 \times 10^{-2}$	$2 \times 10^{-2}$	$4 \times 10^{-4}$
$III$	$2 \times 10^{-2}$	$4 \times 10^{-2}$	$8 \times 10^{-4}$

  Which of the following are correct statements -

$(a)$  Rate constant of the reaction $10^{-4}$

$(b)$  Rate law of the reaction is $k[A][B]$

$(c)$  Rate of reaction increases four times on doubling the concentration of both the reactant

 $A + B \to $ products, it is found that the rate of the reaction is proportional to the concentration of $A,$  but it is independent of the concentration of $B$, then

Which one of the following statement for order of reaction is not correct ?

For the reaction

$2 \mathrm{H}_{2}(\mathrm{g})+2 \mathrm{NO}(\mathrm{g}) \rightarrow \mathrm{N}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})$

the observed rate expression is, rate $=\mathrm{k}_{\mathrm{f}}[\mathrm{NO}]^{2}\left[\mathrm{H}_{2}\right] .$ The rate expression of the reverse reaction is

The following data are for the decomposition of ammonium nitrate in aqueous solution Volume of ....... The order of the reaction is

${A_2} + {B_2} \to 2AB;R.O.R = k{[{A_2}]^a}{[{B_2}]^b}$

Order of reaction with respect to $A_2$ and $B_2$ are respectively