Identify the reaction order for which the rate constant $K = 2.3 \times 10^{-5} \ L \ mol^{-1} \ s^{-1}$.

$A$ reaction involving two different reactants:

The order of the reaction occurring by the following mechanism should be:
$(i)$ $A_2 \to A + A$ (fast)
$(ii)$ $A + B_2 \to AB + B$ (slow)
$(iii)$ $A + B \to AB$ (fast)

For the reaction $A + B \to \text{products}$,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:

$2 \ NO_{(g)} + Cl_{2(g)} \rightleftharpoons 2 \ NOCl_{(g)}$
This reaction was studied at $-10^{\circ} C$ and the following data was obtained:

$Run$	$[NO]_{0}$	$[Cl_{2}]_{0}$	$r_{0}$
$1$	$0.10$	$0.10$	$0.18$
$2$	$0.10$	$0.20$	$0.35$
$3$	$0.20$	$0.20$	$1.40$

$[NO]_{0}$ and $[Cl_{2}]_{0}$ are the initial concentrations and $r_{0}$ is the initial reaction rate.
The overall order of the reaction is ..........
(Round off to the Nearest Integer).

At $345 \ K$,the half-life for the decomposition of a sample of a gaseous compound initially at $55.5 \ kPa$ was $340 \ s$. When the pressure was $27.8 \ kPa$,the half-life was found to be $170 \ s$. The order of the reaction is $......$ [integer answer]