- A$Cl$
- B$Mn$
- C$Np$
- ✓All of these
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$\begin{array}{*{20}{c}}
{\,\,\,\,\,\,\,\,\,\,\,C{H_3}}\\
{\,\,\,|\,\,}\\
{C{H_3} - C{H_2} - CH - C - N{H_2}}\\
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,||}\\
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,O\,\,\,}
\end{array}$ $\xrightarrow[\Delta ]{{B{r_2}/KOH}}\left( A \right)\xrightarrow{\begin{subarray}{l}
(1)\,\,C{H_3}I\,{\text{(excess)}} \\
(2)\,AgOH/\Delta \,
\end{subarray} }$ $(B)$

$[A]$ With increase in temperature, the value of $K$ for exothermic reaction decreases because entropy change of the system is positive
$[B]$ With increase in temperature, the value of $K$ for endothermic reaction increases because unfavourable change in entropy of the surroundings decreases
$[C]$ With increase in temperature, the value of $K$ for endothermic reaction increases because the entropy change of the system is negative
$[D]$ With increase in temperature, the value of $K$ for exothermic reaction decreases because favourable change in entropy of the surrounding decreases