$A_2 + 2\,B \to 2\,AB$

$[A_2]$	$[B]$	${-d\,[A_2]/dt}$
$0.1$	$0.2$	$1 \times {10^{ - 2}}\,M{s^{ - 1}}$
$0.2$	$0.2$	$2 \times {10^{ - 2}}\,M{s^{ - 1}}$
$0.2$	$0.4$	$8 \times {10^{ - 2}}\,M{s^{ - 1}}$

Order of reaction w.r.t. $A_2$ and $B$ are respectively

The rate law of the reaction $2{N_2}{O_5} \to 4N{O_2} + {O_2}$ is

The rate of the reaction becomes twice when the concentration of reactant becomes $8$ times then the order of the reaction is

In a reaction if the concentration of reactant A is tripled, the rate of reaction becomes twenty seven times. What is the order of the reaction ?

For the reaction $A + 2B \to C,$ rate is given by $R$ $ = [A]{[B]^2}$ then the order of the reaction is

When a reaction is progressing