- A$S + K$
- B$S{b_2}{S_3}$
- ✓${K_2}C{r_2}{O_7} + S + $ red $P$
- D${K_2}C{r_2}{O_7} + K + S$
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$CH_3-CH_2-COOH$ $\mathop {\xrightarrow{{(i)\,AgN{O_3}}}}\limits_{(ii)\,B{r_2}/\Delta } $ $[X]$
$[X]$ will be :
In the above reaction $'A'$ is ....
Product $(A)$ of above reaction will be
$\mathrm{Cd}_{(s)}+\mathrm{Hg}_{2} \mathrm{SO}_{4(s)}+\frac{9}{5} \mathrm{H}_{2} \mathrm{O}_{(l)} \rightleftharpoons \mathrm{CdSO}_{4} \cdot \frac{9}{5} \mathrm{H}_{2} \mathrm{O}_{(s)}+2 \mathrm{Hg}_{(l)}$
The value of $\mathrm{E}_{\text {cell }}^{0}$ is $4.315\, \mathrm{~V}$ at $25^{\circ} \mathrm{C}$. If $\Delta \mathrm{H}^{\circ}=-825.2\, \mathrm{~kJ} \,\mathrm{~mol}^{-1}$, the standard entropy change $\Delta \mathrm{S}^{\circ}$ in $\mathrm{J} \,\mathrm{K}^{-1}$ is ........ . (Nearest integer) [Given : Faraday constant $=96487\, \mathrm{C}\, \mathrm{mol}^{-1}$ ]