- A$CH_3-CH_2-Br$
- B$\begin{array}{*{20}{c}}
{C{H_3} - CH - I} \\
{\,|} \\
{\,\,\,\,\,\,\,\,C{H_3}}
\end{array}$ - ✓$CH_3-CH_2-CH_2-Cl$
- D$CH_3-(CH_2)_5-F$
Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.
(Image)
Total number of $\pi$ bonds present in product ' $P$ ' is/are
Cell notation : $M \left|\underset{0.01}{ M ^{2+}} \| \underset{0.0001}{ M ^{2+}}\right| M$
.........$V$ value of $E _{ Cell }^{o}$ is $4$ volt (Given $\frac{ RT }{ F }$ in $10=0.06$ )

$M \mid M ^{2+}$ (saturated solution of a sparingly soluble salt, $\left.MX _2\right) \| M ^{2+}\left(0.001\right.$ mol dm $\left.d ^{-3}\right) \| M$ The emf of the cell depends on the difference in concetration of $M ^{2+}$ ions at the two electrodes. The emf of the cell at $298$ is $0.059 \ V$
$1.$ The solubility product $\left( K _{ sp } ; mol ^3 dm ^{-9}\right)$ of $MX _2$ at $298$ based on the information available the given concentration cell is (take $2.303 \times R \times 298 / F =0.059 \ V$ )
$(A)$ $1 \times 10^{-15}$ $(B)$ $4 \times 10^{-15}$
$(C)$ $1 \times 10^{-12}$ $(D)$ $4 \times 10^{-12}$
$2.$ The value of $\Delta G \left( kJ \ mol ^{-1}\right)$ for the given cell is (take $1 F =96500 \ C \ mol ^{-1}$ )
$(A)$ $-5.7$ $(B)$ $5.7$ $(C)$ $11.4$ $(D)$ $-11.4$
Give the answer question $1$ and $2.$