- AEthylene glycol
- BOxalic acid
- CGlycerol
- ✓Tartaric acid
So it is optically active.
$\mathop {\begin{array}{*{20}{c}}
{\begin{array}{*{20}{c}}
{\,\,\,\,OH} \\
| \\
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,H - {C^*} - COOH\,\,\,} \\
|
\end{array}} \\
{\,\,\,\,\,\,\,\,\,\,\,\,\,H - {C^*} - COOH} \\
| \\
{\,\,\,OH}
\end{array}}\limits_{{\text{Tartaricacid}}} $
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Benzene $(C_6H_6)$ $+\,C{{H}_{3}}-CH=C{{H}_{2}}\,\xrightarrow{{{H}^{\oplus }}}A\xrightarrow{{{O}_{2}}}B$ $\xrightarrow{{{H}^{\oplus }}\,/\,\Delta }C+$$\begin{matrix}
O \\
|| \\
C{{H}_{3}}-C-C{{H}_{3}} \\
\end{matrix}$
The structure of intermediate compound $'B'$ will be
(Image)
Pre-exponential factors for the forward and backward reactions are $10^{15} \mathrm{~s}^{-1}$ and $10^{11} \mathrm{~s}^{-1}$, respectively. If the value of $\log \mathrm{K}$ for the reaction at $500 \mathrm{~K}$ is $6$ , the value of $\left|\log \mathrm{k}_{\mathrm{b}}\right|$ at $250 \mathrm{~K}$ is $\qquad$
$[\mathrm{K}=$ equilibrium constant of the reaction
$\mathrm{k}_{\mathrm{f}}=$ rate constant of forward reaction
$\mathrm{k}_{\mathrm{b}}=$ rate constant of backward reaction]
