Given below are two statements : Statement I: The rate law for the reaction (A+B arrow 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

Correct answer: 0 r=K[A]^2| B| if conc. are doubled aligned & r^ =K[2 A]^2[2 B]^1 & r^ =8 r x=8 aligned aligned & Zero order, y=0 & x+y=8 aligned

JEE Main 20249 AprilMorning Shift

JEE Main 2024 · 9 April · Morning Shift · Chemistry · Chemical Kinetics

Given below are two statements : Statement I: The rate law for the...

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 : Given below are two statements : Statement I: The rate law for the reaction (A+B arrow C) is rate (r)=k[A]^2[B] . When

The figure is showing "the variation in concentration against time plot" for a "

y

" order reaction. The Value of

x+y

is ______

\mathrm{r}=\mathrm{K}[\mathrm{A}]^2|\mathrm{ B}|

if conc. are doubled

\begin{aligned} & \mathrm{r}^{\prime}=\mathrm{K}[2 \mathrm{ A}]^2[2 \mathrm{ B}]^1 \\ & \mathrm{r}^{\prime}=8 \mathrm{r} \Rightarrow \mathrm{x}=8 \end{aligned}

\begin{aligned} & \Rightarrow \text{ Zero order, } y=0 \\ & x+y=8\end{aligned}