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 :
The figure is showing "the variation in concentration against time plot" for a " $y$ " order reaction. The Value of $x+y$ is ______

Question

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 :

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

Aicharya · Accepted Answer

$\mathrm{r}=\mathrm{K}[\mathrm{A}]^2|\mathrm{~B}|$ if conc. are doubled $\begin{aligned} & \mathrm{r}^{\prime}=\mathrm{K}[2 \mathrm{~A}]^2[2 \mathrm{~B}]^1 \\ & \mathrm{r}^{\prime}=8 \mathrm{r} \Rightarrow \mathrm{x}=8 \end{aligned}$

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

Given below are two statements : Statement I: The rate law for the reaction \(A+B \rightarrow C\) is rate…

Solution