Chemistry - Chemical Kinetics Question with Solution | TestHub

Given below are two statements :

Statement I : The rate law for the reaction $\mathrm{A}+\mathrm{B}\to \mathrm{C}$ is rate $(\mathrm{r})=\mathrm{k}[\mathrm{A}{]}^2[\mathrm{B}]$. When the concentration of both A and $B$ is doubled, the reaction rate is increased " $x$ " times.

Statement II : For the reaction : $\mathrm{R}\to \mathrm{S}+\mathrm{T}$

The figure is showing "the variation in concentration against time plot" for a " y " order reaction. The value of $x+y$ is $\_\_\_\_$ .