Consider the reaction, $2\mathrm{A}+\mathrm{B}⟶\mathrm{C}+\mathrm{D}$. If the rate expression is $\mathrm{r}=\mathrm{K}{\left[\mathrm{A}\right]}^2{\left[\mathrm{B}\right]}^0$ and if volume is reduced to $\frac{1}{3}$, the rate of reaction will increase

Assuming an elementary reaction ${\mathrm{H}}_2{\mathrm{O}}_2+3{ \mathrm{F}}^{-}+2{\mathrm{H}}^{+}$$⟶2{\mathrm{H}}_2\mathrm{O}+{\mathrm{I}}_3^{-}$. The effect on the rate of this reaction brought about by doubling the concentration of $1^{-}$ without changing the order

Consider the following in respect of zero order reaction

I. ${\mathrm{t}}_{1/2}$ is directly proportional to the initial concentration

II. Time taken for the completion of the reaction is twice its ${\mathrm{t}}_{1/2}$

III. Concentration of the reactant decreases linearly with time

Which of the statements given above are correct?