Q57. Given below are two statements : Statement I : The rate law for the reaction $A + B \rightarrow C$ is rate $( r ) = k [ A ] ^ { 2 } [ B ]$ . When the concentration of both A and B is doubled, the reaction rate is increased " $x$ " times. Statement II : [Figure] The figure is showing "the variation in concentration against time plot" for a " $y$ " order reaction. The Value of $x + y$ is $\_\_\_\_$
Q57. Given below are two statements : Statement I : The rate law for the reaction $A + B \rightarrow C$ is rate $( r ) = k [ A ] ^ { 2 } [ B ]$ . When the concentration of both A and B is doubled, the reaction rate is increased " $x$ " times. Statement II :\\
\includegraphics[max width=\textwidth, alt={}, center]{4e2e81bd-4b90-4bb9-aa98-645235480371-10_364_384_260_226}
The figure is showing "the variation in concentration against time plot" for a " $y$ " order reaction. The Value of $x + y$ is $\_\_\_\_$\\