- A$1\,L$ of $0.5\, M \,H_2SO_4$
- B$49\, gm$ of $H_2SO_4$
- C$0.5\, mol$ of $H_2\, gas$
- ✓All of the above
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$CHC{l_3}\,\xrightarrow[{Zn/HCl\,\,(alc.)}]{{ +\, 2H}}$
$CHC{l_3}\,\xrightarrow[{Zn/HCl\,\,(aq)}]{{ + \,4H}}$
$CHC{l_3}\,\xrightarrow[{Zn/{H_2}O}]{{ + \,6H}}$
$\mathrm{Cd}_{(s)}+\mathrm{Hg}_{2} \mathrm{SO}_{4(s)}+\frac{9}{5} \mathrm{H}_{2} \mathrm{O}_{(l)} \rightleftharpoons \mathrm{CdSO}_{4} \cdot \frac{9}{5} \mathrm{H}_{2} \mathrm{O}_{(s)}+2 \mathrm{Hg}_{(l)}$
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 $=96487\, \mathrm{C}\, \mathrm{mol}^{-1}$ ]