For the reaction $2A + B \rightarrow \text{Product}$,the half-life remains unchanged when the concentration of $A$ is doubled. When the concentration of $B$ is doubled,the rate of reaction increases by a factor of $2$. What is the unit of the rate constant for this reaction?

$A$ study of chemical kinetics of the reaction $A + B \to$ Products,gave the following data at $25 \ ^oC$.

$Exp. \ No.$	$[A]$	$[B]$	$Rate$
$1.$	$1.0$	$0.15$	$4.2 \times 10^{-6}$
$2.$	$2.0$	$0.15$	$8.4 \times 10^{-6}$
$3.$	$1.0$	$0.20$	$5.6 \times 10^{-6}$

Find out the rate law.

If in a certain reaction,two different reactants take part,then:

If $a$ is the initial concentration of the reactant,the half-life period of the reaction of $n^{th}$ order is inversely proportional to

Higher order $(> 3)$ reactions are rare due to:

State whether the following statements are true $(T)$ or false $(F)$.
$(a)$ In a pseudo first order reaction,the rate and rate constant are determined with respect to the reactant present in lower concentration.
$(b)$ The hydrolysis of an ester is carried out in the presence of an excess of water in an acidic medium.
$(c)$ The hydrolysis of an ester is a second order reaction.