The $E_a$ of a reaction in presence of a catalyst is $4.15 kJ mo{l}^{-1}$ and in absence of a catalyst is $8.3 kJ mo{l}^{-1}$ . What is slope of the plot of $lnk vs\frac{1}{T}$ in the absence of catalyst

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:

The reaction of ${\mathrm{NO}}_2 \left(\mathrm{g}\right)$ and ${\mathrm{O}}_3 \left(\mathrm{g}\right)$ is first order in ${\mathrm{NO}}_2 \left(\mathrm{g}\right)$ and ${\mathrm{O}}_3 \left(\mathrm{g}\right)$

$2{\mathrm{NO}}_2 \left(\mathrm{g}\right)+{\mathrm{O}}_3 \left(\mathrm{g}\right)⟶{\mathrm{N}}_2{\mathrm{O}}_5 \left(\mathrm{g}\right)+{\mathrm{O}}_2 \left(\mathrm{g}\right)$

The reaction can take place by mechanism:

$\mathrm{I}:{\mathrm{NO}}_2+{\mathrm{O}}_3\stackrel{\mathrm{sbw}}{⟶}{\mathrm{NO}}_3+{\mathrm{O}}_2$

${\mathrm{NO}}_3+{\mathrm{NO}}_2\stackrel{\text{ fast }}{⟶}{\mathrm{N}}_2{\mathrm{O}}_5$

$\mathrm{II}:{\mathrm{O}}_3\underset{{\mathrm{K}}_{\mathrm{b}}}{\overset{{\mathrm{k}}_{\mathrm{a}}\text{ fast }}{\rightleftharpoons }}{\mathrm{O}}_2+\left[\mathrm{O}\right]$

${\mathrm{NO}}_2+\mathrm{O}\stackrel{\text{ slow }}{⟶}{\mathrm{NO}}_3$

${\mathrm{NO}}_3+{\mathrm{NO}}_2\stackrel{\text{ fast }}{⟶}{\mathrm{N}}_2{\mathrm{O}}_5$

Select correct mechanism.

A substance undergoes first order decomposition. The decomposition follows two parallel first order reactions as :

$$\begin{gathered} {\mathrm{k}}_1=1.26\times {10}^{-4} {\mathrm{s}}^{-1} \\ {\mathrm{k}}_2=3.8\times {10}^{-5} {\mathrm{s}}^{-1} \end{gathered}$$

The percentage distribution of $\mathrm{B}$ and $\mathrm{C}$ are