The graph plotted between concentration versus time
 

The rate law of a reaction between the substances $\mathrm{A}$ and $\mathrm{B}$ is given by, rate $=\mathrm{k}{\left[\mathrm{A}\right]}^{\mathrm{n}}{\left[\mathrm{B}\right]}^{\mathrm{m}}$. On doubling the concentration of $A$ and making the volume of $\mathrm{B}$ half the ratio of new rate to the earlier rate of reaction will be

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

The late law for the reaction

$\mathrm{RCl}+\mathrm{NaOH}\left(\mathrm{aq}\right)⟶\mathrm{ROH}+\mathrm{NaCl}$

is given by Rate $=\mathrm{k}\left[\mathrm{RCl}\right]$. The rate of reaction will be