In the following gaseous phase first order reaction, $\mathrm{A}\left(\mathrm{g}\right)⟶2 \mathrm{B}( \mathrm{g})+\mathrm{C}\left(\mathrm{g}\right)$ initial pressure was found to be $400 \mathrm{mm}$, and it changed to $1000 \mathrm{mm}$ after $20 \min \mathrm{.}$ Then the correct statements are :-

For the reaction ${\mathrm{CH}}_4+{\mathrm{Br}}_2⟶{\mathrm{CH}}_3\mathrm{Br}+\mathrm{HBr}$, the experimental data require the following rate equation:

$\frac{\mathrm{d}}{\mathrm{dt}}\left[{\mathrm{CH}}_3\mathrm{Br}\right]=\frac{{\mathrm{k}}_1\left[{\mathrm{CH}}_4\right]\left[{\mathrm{Br}}_2\right]}{1+{\mathrm{k}}_2\left[\mathrm{HBr}\right]/\left[{\mathrm{Br}}_2\right]}$

Which of the following is/are true regarding this?

Which of the following statements are true regarding the $\log \mathrm{K} \mathrm{vs} 1/\mathrm{T}$ plot shown in the given diagram?

If the rate of reaction $2{\mathrm{SO}}_2 \left(\mathrm{g}\right)+{\mathrm{O}}_2 \left(\mathrm{g}\right)\stackrel{\mathrm{Pi}}{⟶}2{\mathrm{SO}}_3 \left(\mathrm{g}\right)$ is given by: Rate$=\mathrm{K}\frac{\left[{\mathrm{SO}}_2\right]}{{\left[{\mathrm{SO}}_3\right]}^{1/2}}$

Which statements are correct?