r=K[A]2∣ B∣ if conc. are doubled $\begin{aligned}
& \mathrm{r}^{\prime}=\mathrm{K}[2 \mathrm{A}]^2[2 \mathrm{B}]^1 \
& \mathrm{r}^{\prime}=8 \mathrm{r} \Rightarrow \mathrm{x}=8
\end{aligned}$ 
⇒ Zero order, y=0x+y=8
JEE Main 2024 — Chemistry Physical Chemistry
2024integerhard
Given below are two statements : Statement I: The rate law for the reaction A+B→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 : 
The figure is showing "the variation in concentration against time plot" for a " y " order reaction. The Value of x+y is ______
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Held on 9 Apr 2024 · Verified 6 Jul 2026.
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