During Kinetic study of reaction $2 A+B \rightarrow C+D$, the following results were obtained :

	$A[M]$	$B[M]$	initial rate of formation of $D$
$i$	$0.1$	$0.1$	$6.0 \times 10^{-3}$
$ii$	$0.3$	$0.2$	$7.2 \times 10^{-2}$
$ii$	$0.3$	$0.4$	$2.88 \times 10^{-1}$
$iv$	$0.4$	$0.1$	$2.40 \times 10^{-2}$

Based on above data, overall order of the reaction is $\qquad$

The unit of rate constant for a zero order reaction is

For a chemical reaction....can never be a fraction

Following is the rate constant of reaction what is the overall order of reaction ?

$(a)$ $6.66 \times 10^{-3} \,s ^{-1}$

$(b)$ $4.5 \times 10^{-2} \,mol ^{-1} \,L \,s ^{-1}$

Consider following two reaction,

$A \to {\text{Product ;}}\,\, - \frac{{d[A]}}{{dt}} = {k_1}{[A]^o}$

$B \to {\text{Product ;}}\,\, - \frac{{d[B]}}{{dt}} = {k_2}{[B]}$

Units of $k_1$ and $k_2$ are expressed in terms of molarity $(M)$ and time $(sec^{-1})$ as

The unit of rate constant of second order reaction is usually expressed as