$A$ chemical reaction takes place in two steps as follows:
$(i) \ NO_2Cl_{(g)} \xrightarrow{K_1} NO_{2(g)} + Cl_{(g)}$
$(ii) \ NO_2Cl_{(g)} + Cl_{(g)} \xrightarrow{K_2} NO_{2(g)} + Cl_{2(g)}$
Identify the reaction intermediate.

Give two examples of zero-order reactions and two examples of first-order reactions.

The half-life for a second-order reaction is $30 \ min$. If the initial concentration is $0.1 \ M$,then the value of the rate constant will be $............ \ M^{-1} \ min^{-1}$.

$2 \ NO_{(g)} + Cl_{2(g)} \rightleftharpoons 2 \ NOCl_{(g)}$
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).

For a reaction $A + B \rightarrow \text{product}$,if $[A]$ is doubled keeping $[B]$ constant,the rate of reaction doubles. Calculate the order of reaction with respect to $A$.

The reaction $2NO_{(g)} + O_{2(g)} \rightleftharpoons 2NO_{2(g)}$ is of first order. If the volume of the reaction vessel is reduced to $1/3$ of its original volume,the rate of reaction would be .......... times.