For the reaction $2NO_2 + F_2 \to  2NO_2F$, following mechanism has been provided :
$N{O_2} + {F_2}\xrightarrow{{slow}}N{O_2}F + F$
$N{O_2} + {F_2}\xrightarrow{{fast}}N{O_2}F$
Thus rate expression of the above reaction can be written as

For reaction

$Cl_2(aq) + H_2S(aq) \to S(s) + 2H^+(aq) + 2Cl^-(aq)$ rate law is $r = K[Cl_2][H_2S]$
then which of these mechanism is/are consistent with this rate law

$(A)\, H_2S \rightleftharpoons  H^+ + HS^-$ (fast)

         $Cl_2 + HS^-\to 2Cl^-+ H^+ + S$ (slow)

$(B)\, Cl_2 + H_2S \to H^+ + Cl^-+ Cl^+ + HS^-$ (slow)

          $Cl^+ + HS^-\to H^+ + Cl^-+ S$ (fast)

For a reaction $A \to B$, the rate of reaction quadrupled when the concentration of $A$  is doubled. The rate expression of the reaction is $r = K{(A)^n}$. when the value of $n$ is

For the reaction $3\,{A_{\,(g)\,}}\,\xrightarrow{K}\,{B_{(g)}}\, + \,\,{C_{(g)\,,}}K$ is ${10^{ - 14}}\,L/mol.\min .$ if $(A) = 0.5\,M$ then the value of $ - \frac{{d(A)}}{{dt}}$ (in $M / sec$ ) is.

If the half life period of a reaction is inversely proportional to the initial concentration, the order of the reaction is

The reaction, ${N_2}{O_5} \longrightarrow 2NO + \frac{1}{2}\,{O_2}$ is of first order for $N_2O_5$ with rate constant $6.2 \times 10^{-4}\, s^{-1}$. what is the value of rate of reaction when $[N_2O_5] = 1.25\, mol\, L^{-1}$