- A$B{r_2}/KOH$
- B$HCl{O_4}$
- ✓$HN{O_2}$
- D$N{H_3}$
$\mathop {{{(C{H_3}C{H_2})}_2}NH + HN{O_2}}\limits_{{2^o}} \to $
$\mathop {{{(C{H_3}C{H_2})}_2}N - N = O}\limits_{{\rm{Nitroso}}\,\,{\rm{amine}}} + {H_2}O$
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$\begin{array}{*{20}{c}} {\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,OH} \\ {\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,|} \\ {( \pm )\,\,C{H_3} - C{H_2} - CH - C{H_3}} \end{array}$ $\xrightarrow[\Delta ]{{{H_3}P{O_4}}}P\,\xrightarrow[{Ni}]{{{D_2}}}Q$
Which of the following compounds can be $A$ ?
Statement $I$ : The rate law for the reaction $A+B \rightarrow C$ is rate $(r)=k[A]^2[B]$. When the concentration of both $\mathrm{A}$ and $\mathrm{B}$ is doubled, the reaction rate is increased " $\mathrm{x}$ " times.
Statement $II$ :
(Image)
The figure is showing "the variation in concentration against time plot" for a $"y"$ order reaction. The value of $x+y$ is . . . . . . 