The first-order rate constant $\mathrm{k}$ is related to temp. $\mathrm{logk}=15.0-\left(\frac{{10}^6}{\mathrm{T}}\right)$ Which of the following pair of values is correct?

The reaction of hydrogen and iodine monochloride is represented by the equation:

${\mathrm{H}}_2\left(\mathrm{g}\right)+2\mathrm{ICl}\left(\mathrm{g}\right)⟶2\mathrm{HCl}\left(\mathrm{g}\right)+{\mathrm{I}}_2\left(\mathrm{g}\right)$

This reaction is first-order in ${\mathrm{H}}_2\left(\mathrm{g}\right)$ and also first-order in $\mathrm{ICl}\left(\mathrm{g}\right)$. Which of these proposed mechanisms

can be consistent with the given information about this reaction?

Mechanism $\mathrm{I}$: ${\mathrm{H}}_2\left(\mathrm{g}\right)+2\mathrm{ICl}\left(\mathrm{g}\right)⟶2\mathrm{HCl}\left(\mathrm{g}\right)+{\mathrm{I}}_2\left(\mathrm{g}\right)$ 

Mechanism $\mathrm{II}$: ${\mathrm{H}}_2\left(\mathrm{g}\right)+\mathrm{ICl}\left(\mathrm{g}\right)\stackrel{\mathrm{Slow}}{⟶}\mathrm{HCl}\left(\mathrm{g}\right)+\mathrm{HI}\left(\mathrm{g}\right)$

$\mathrm{Hl}\left(\mathrm{g}\right)+\mathrm{ICl}\left(\mathrm{g}\right)\stackrel{\text{ fast }}{⟶}\mathrm{HCl}\left(\mathrm{g}\right)+{\mathrm{I}}_2\left(\mathrm{g}\right)$

Following mechanism has been proposed for a reaction.

$2\mathrm{A}+\mathrm{B}\to \mathrm{D}+\mathrm{E}$

Step$-1 \mathrm{A}+\mathrm{B}\to \mathrm{C}+\mathrm{D}$ (slow)

Step$-2 \mathrm{A}+\mathrm{C}\to \mathrm{E}$ (Fast)

The rate law expression for the reaction is:

The following mechanism has been proposed for a reaction:

$2\mathrm{A}+\mathrm{B}⟶\mathrm{D}+\mathrm{E}$ $\mathrm{K}=2\times {10}^{-1}{\mathrm{It}}^2{\mathrm{mol}}^{-2}{\sec }^{-1}$

$\mathrm{A}+\mathrm{B}⟶\mathrm{C}+\mathrm{D}$ $\mathrm{K}=1.5\times {10}^{-6}\mathrm{It}\text{/mol sec }$

$\mathrm{A}+\mathrm{C}⟶\mathrm{E}$ $\mathrm{K}=2\times {10}^{-3}\mathrm{It}/\mathrm{mol} \sec$

The rate law expression for the reaction is: