For the non - stoichimetre reaction $2A + B \rightarrow C + D,$ the following kinetic data were obtained in three separate experiments, all at $298\, K.$

Initial Concentration $(A)$	Initial Concentration $(A)$	Initial rate of formation of $C$ $(mol\,L^{-1}\,s^{-1})$
$0.1\,M$	$0.1\,M$	$1.2\times 10^{-3}$
$0.1\,M$	$0.2\,M$	$1.2\times 10^{-3}$
$0.2\,M$	$0.1\,M$	$2.4 \times 10^{-3}$

The rate law for the formation of $C$ is :

Select the rate law that corresponds to the data shown for the following reaction $A+ B\to C$

The hypothetical reaction : $2A + B \to C + D$ is catalyzed by $E$ as indicated in the possible mechanism below -

Step$-1$ : ${\text{A  +  E }} \rightleftharpoons AE$ (fast)

Step$-2$ :${\text{AE  +  A }} \to {A_2} + E$ (slow)

Step$-3$ :${{\text{A}}_2}{\text{ +  B }} \to {\text{D}}$ (fast)

what rate law best agrees with this mechanism

Select the rate law for reaction $A + B \longrightarrow C$

The rate of reaction, $A + B + C \longrightarrow P$ is given by

$r = \frac{{ - d\left[ A \right]}}{{dt}} = K\,{\left[ A \right]^{\frac{1}{2}}}\,{\left[ B \right]^{\frac{1}{2}}}\,{\left[ C \right]^{\frac{1}{4}}}$

The order of reaction is

If doubling the initial concentration of reactant doubles $t_{1/2}$ of reaction, the order of reaction is