$2 NO +2 H _{2} \rightarrow N _{2}+2 H _{2} O$

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 $\left(\frac{- dp }{ dt }\right) /( kPa / s )$
$1$	$65.6$	$40.0$	$0.135$
$2$	$65.6$	$20.1$	$0.033$
$3$	$38.6$	$65.6$	$0.214$
$4$	$19.2$	$65.6$	$0.106$

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

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

If a reaction has the experimental rate expression rate $= K [A]^2[B]$, if the concentration of $A$ is doubled and the concentration of $B$ is halved, the what happens to the reaction rate

For reaction $2A + B \to $ products, the active mass of $ B $ is kept constant and that of $A$ is doubled. The rate of reaction will then

For a certain reaction the expression for half life is $t \propto \frac{1}{{{a^{n - 1}}}}$ then the order of reaction is

The rate of the reaction, $2NO + Cl_2 \rightarrow 2NOCl$ is given by the rate equation rate $= k[NO]^2[Cl_2].$ The value of the rate constant can be increased by