For the reaction $A + 2B \longrightarrow C$,the reaction rate is doubled if the concentration of $A$ is doubled. The rate is increased by four times when concentrations of both $A$ and $B$ are increased by four times. The order of the reaction is

The rate equation for the reaction $2A + B \to C$ is found to be: $\text{rate} = k[A][B]$. The correct statement in relation to this reaction is that the

Consider the following reactions:
$A$ $\rightarrow P_1; B$ $\rightarrow P_2; C$ $\rightarrow P_3; D$ $\rightarrow P_4$
The orders of the above reactions are $a, b, c,$ and $d,$ respectively. The following graph is obtained when $\log[\text{rate}]$ vs. $\log[\text{conc.}]$ are plotted:
Among the following,the correct sequence for the order of the reactions is:

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

Initial $[A_2]$	Initial $[B_2]$	$R.O.R. (r) \ M s^{-1}$
$0.2$	$0.2$	$0.04$
$0.1$	$0.4$	$0.04$
$0.2$	$0.4$	$0.08$

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

By “the overall order of a reaction”,we mean

The given reaction $2NO + O_2 \to 2NO_2$ is an example of