A graph is plotted between log $\mathrm{K}$ versus $\frac{1}{\mathrm{T}}$ for calculation of activation energy $\left({\mathrm{E}}_{\mathrm{a}}\right)$. The correct plot is

Given the hypothetical reaction mechanism

$\mathrm{A}\stackrel{\mathrm{I}}{⟶}\mathrm{B}\stackrel{\mathrm{II}}{⟶}\mathrm{C}\stackrel{\mathrm{III}}{⟶}\mathrm{D}\stackrel{\mathrm{IV}}{\to } \mathrm{E}$ and the rate as

The rate determining step is

For the chemical reaction

$2{\mathrm{O}}_3⟶3{\mathrm{O}}_2$, the reaction proceeds as follows

${\mathrm{O}}_3\rightleftharpoons {\mathrm{O}}_2+\mathrm{O}$ (Fast)

$\mathrm{O}+{\mathrm{O}}_3⟶2{\mathrm{O}}_2$, (Slow)

the rate law expression should be given as

For a reversible reaction, $\mathrm{A}\rightleftharpoons \mathrm{B}$, which one of the following statement is wrong from the given energy profile diagram?

Which of the following expression is correct for the rate of reaction given below ?

$5{\mathrm{Br}}^{-}\left(\mathrm{aq}\right)+{\mathrm{BrO}}_3^{-}\left(\mathrm{aq}\right)+6{\mathrm{H}}^{+}\left(\mathrm{aq}\right)⟶3{\mathrm{Br}}_2\left(\mathrm{aq}\right)+3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

A graph is plotted between log $\mathrm{K}$ versus $\frac{1}{\mathrm{T}}$ for calculation of activation energy $\left({\mathrm{E}}_{\mathrm{a}}\right)$. The correct plot is