If the value of the rate constant $K = 2.3 \times 10^{-5} \ L \ mol^{-1} \ s^{-1}$,then identify the reaction order:

The reaction $2NO + Br_2 \rightarrow 2NOBr$ follows the mechanism given below:
$(I)$ $NO + Br_2 \rightleftharpoons NOBr_2$ ........ Fast
$(II)$ $NOBr_2 + NO \rightarrow 2NOBr$ ......... Slow
The overall order of this reaction is

For a zero order reaction,will the molecularity be equal to zero? Explain.

For a reaction,$AB_5 \to AB + 4B$,the rate can be expressed in the following ways:
$-\frac{d[AB_5]}{dt} = K[AB_5]$ ; $\frac{d[B]}{dt} = K_1[AB_5]$
What is the correct relation between $K$ and $K_1$?

From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant.
$(iii)$ $CH_{3}CHO_{(g)} \rightarrow CH_{4(g)} + CO_{(g)} \quad$ Rate $= k[CH_{3}CHO]^{3/2}$

$2 \ NO + 2 \ H_2 \rightarrow N_2 + 2 \ H_2O$
The above reaction has been studied at $800^{\circ} C$. The related data are given in the table below.

Reaction serial number	Initial pressure of $H_2$ / $kPa$	Initial Pressure of $NO$ / $kPa$	Initial rate $(-\frac{dp}{dt}) / (kPa \ s^{-1})$
$1$	$65.6$	$40.0$	$0.135$
$2$	$65.6$	$20.1$	$0.033$
$3$	$38.6$	$65.6$	$0.214$
$4$	$19.2$	$65.6$	$0.106$

The order of the reaction with respect to $NO$ is $...........$