Slope of the graph $\ln [\mathrm{A}{]}_{\mathrm{t}}$ versus $\mathrm{t}$ for first order reaction is

The reaction, $3{\mathrm{ClO}}^{\ominus }\to {\mathrm{ClO}}_3^{\ominus }+2{\mathrm{Cl}}^{\ominus }$ occurs in two steps,
(i) $2{\mathrm{ClO}}^{-}⟶{\mathrm{ClO}}_2^{\ominus }$

(ii) ${\mathrm{ClO}}_2^{\ominus }+{\mathrm{ClO}}^{\ominus }⟶{\mathrm{ClO}}_3^{\ominus }+{\mathrm{Cl}}^{\ominus }$

The reaction intermediate is

For the reaction,

${\mathrm{N}}_2( \mathrm{g})+3{\mathrm{H}}_2( \mathrm{g})⟶2{\mathrm{NH}}_3( \mathrm{g})$

what is the relationship among $\frac{\mathrm{d}\left[{\mathrm{N}}_2\right]}{\mathrm{dt}}$, $\frac{\mathrm{d}\left[{\mathrm{H}}_2\right]}{\mathrm{dt}}$ and $\frac{\mathrm{d}\left[{\mathrm{NH}}_3\right]}{\mathrm{dt}}$?

For the reaction,

${\mathrm{CH}}_3\mathrm{Br}\left(\mathrm{aq}\right)+{\mathrm{OH}}^{-}\left(\mathrm{aq}\right)⟶{\mathrm{CH}}_3{\mathrm{OH}}^{\ominus }\left(\mathrm{aq}\right)+{\mathrm{Br}}^{\ominus }\left(\mathrm{aq}\right)$, rate law is rate $=\mathrm{k}\left[{\mathrm{CH}}_3\mathrm{Br}\right]\left[{\mathrm{OH}}^{\ominus }\right]$

How does reaction rate changes if $\left[{\mathrm{OH}}^{\ominus }\right]$ is decreased by a factor of $5$?
 

For the reaction,

${\mathrm{CH}}_3\mathrm{Br}\left(\mathrm{aq}\right)+{\mathrm{OH}}^{-}\left(\mathrm{aq}\right)⟶{\mathrm{CH}}_3{\mathrm{OH}}^{\ominus }\left(\mathrm{aq}\right)+{\mathrm{Br}}^{\ominus }\left(\mathrm{aq}\right)$, rate law is rate $=\mathrm{k}\left[{\mathrm{CH}}_3\mathrm{Br}\right]\left[{\mathrm{OH}}^{\ominus }\right]$

What is change in rate if concentrations of both reactants are doubled?