For a second order reaction plots are made for $\frac{1}{[ \mathrm{A}]}$ vs time for the reaction, $2 \mathrm{A}⟶$ Product. Pick up the correct sentences. $[\mathrm{K}=$ Rate constant of $\mathrm{A}]$

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?