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

From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.

$(iv)$ $C _{2} H _{5} Cl ( g ) \rightarrow C _{2} H _{4}( g )+ HCl ( g ) \quad$ Rate $=k\left[ C _{2} H _{5} Cl \right]$

Which of the following oxides of nitrogen will be the most stable one

 $A + B \to $ products, it is found that the rate of the reaction is proportional to the concentration of $A,$  but it is independent of the concentration of $B$, then

What is molecularity of a relation ? Explain its types by examples.

In a reaction, $A + B \rightarrow$ product, rate is doubled when the concentration of $B$ is doubled, and rate increases by a factor of $8$ when the concentration of both the reactants $(A$ and $B)$ are doubled, rate law for the reaction can be written as