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

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

The rate equation for the reaction $2A + B \to C$ is found to be : rate $ = k[A][B]$. The correct statement in relation to this reaction is that the

For the reaction $2HI$ $\rightleftharpoons$ ${H_2} + {I_2}$, the rate of the reaction is proportional to ${[HI]^2}$. This means that the reaction is

Reaction : $KCl{O_3} + 6FeS{O_4} + 3{H_2}S{O_4} \to $ $KCl + 3F{e_2}{\left( {S{O_4}} \right)_3} + 3{H_2}O$

Which is True $(T)$ and False $(F)$ in the following sentence ?

The order of this reaction is $1$.

Assertion : The kinetics of the reaction -

$mA + nB + pC \to m' X + n 'Y + p 'Z$

obey the rate expression as $\frac{{dX}}{{dt}} = k{[A]^m}{[B]^n}$.

Reason : The rate of the reaction does not depend upon the concentration of $C$.